- published: 16 Nov 2014
- views: 433
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Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, which consists of hydrated iron(III) oxide (ferric oxide). Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O.
This video is targeted to blind users.
Attribution:
Article text available under CC-BY-SA
Creative Commons image source in video
Full Details : http://dscript.org/homegrown-ironii-oxide
This video demonstrates how to produce some home-grown Iron(II) Oxide, otherwise known as ferrous oxide, or black rust.
Iron(II) Oxide is produced when Iron oxidises but does not have enough oxygen to get all the way up to Iron(III) Oxide. The oxidation process can be stalled and it will happily oxidise to black rust and stop there under the right conditions.
The simplest way to do this is to put some iron in a sealed container. Fill it will heavily saturated salt water and let it sit for a few days. It helps if the iron is "pre-rusted" a bit to "jump start" the rusting process.
The heavy concentration of salt will keep the levels of dissolved gases very low and deprive the iron of easy access to oxygen.
As the iron rusts in low oxygen environment, it becomes Iron(II) Oxide and forms a layer of fine particulate on the bottom of the container.
This stuff is used for many things, often as black colouring and dye.
Concentrating it is a simple matter of using magnets, and at any point it can either be stored is it's salt water solution or dehydrated and bound to/into forming salt crystals.
This is for DIY and experimental purposes only, please don't oxide iron or any other metals, excessively or unnecessarily, it takes alot of energy to reduce the original metal oxides into the pure metal form. every time you oxidise metals you are undoing alot of hard work.
I plan to use this stuff in my water circuits. It will allow me to add magnetic responsivity into my fluid environment. Not sure if it will be used to "pump" water, open/close "gates" or various other applications. we will have to see what works ;)
- published: 15 Jul 2013
- views: 1359
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage
So I revisited the salt storage method for my ferrous oxide. I did a "harvest" on one of my production bottles and got a decent amount of ferrous oxide. so I decided to experiment.
I figured there was enough for 3 good samples.
The first I did a hard boil down of the salt-iron(II)oxide mixture - this produce a nice marble textured salt bed. On first glace it seems promising, the iron oxide is dispersed relatively well.
For the second I added a bunch of vinegar -
- published: 16 Jul 2013
- views: 625
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide, which is rare, and iron(III) oxide also known as hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic. Its most extensive use is as a black pigment which is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production.
This video is targeted to blind users.
Attribution:
Article text available under CC-BY-SA
Creative Commons image source in video
- published: 22 Oct 2015
- views: 143
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do organisms compete with chemical oxidation?
ESD welcomes George W. Luther, Ph.D. (Univ. of Delaware)
The oxidation of aqueous Fe(II) to Fe(III) solids is of great significance to Earth history including banded iron formation (BIFs) and the rise of O2 in waters and the atmosphere. The chemical oxidation of aqueous Fe(II) in air saturated solutions is facile at circumneutral pH, but O2 arises mainly from photosynthetic activity. There are currently three theories on how microbes could have contributed to Fe(III) precipitation: (1) oxygenic photosynthesis, coupled to abiotic Fe oxidation, (2) aerobic (anaerobic?) Fe oxidation by iron oxidizing bacteria (FeOB), and (3) anoxygenic photosynthesis, with Fe as an electron donor (photoferrotrophs). Using kinetic data obtained in the field as well as in the laboratory with in situ microelectrode techniques developed in our lab, it is now possible to discriminate between chemical Fe(II) oxidation and these microbially based processes in real time. Field data will be shown from diverse sites including Yellowstone National Park where groundwater, rich in Fe(II) and Mn(II) but with little or no O2, enter oxygenated systems. In the case of FeOB, their importance in Fe(II) oxidation increases at low O2 concentrations. Thermodynamic calculations for the first electron transfer between the metal ions, Fe(II) and Mn(II),with O2 over pH gives insight to the distribution of these metals in BIFs and their biogeochemical behavior.
- published: 05 Mar 2015
- views: 57
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following equation :
10 FeSO4 + 2 KMnO4 + 8 H2SO4 → 5 Fe2(SO4)3 + K2SO4 + 2 MnSO4 + 8 H2O
Firs 98% sulfuric acid is added to 200 ml water in the Erlenmeyer flask and the two are mixed together.
Then potassium permanganate solution is added.
When the two are ready iron(II) sulfate solution is added to the flask causing an instantaneous change in color from the deep violet of permanganate ion to the light green - white of the iron(III) sulfate.
This reaction is much faster than other because according to the collision theory only some collision are effective depending on the form of the molecule the temperature and the concentration .
At the same concentration this reaction is much faster than other because of the nature of iron(II) ion that, being spherical, is reactive towards all oxidizing ions or molecules coming from all directions.
WARNING IRON(II) SULFATE IS IRRITATING TOWARDS SKIN SULFURIC ACID IS CORROSIVE AND POTASSIUM PERMANGANATE IS HIGHLY TOXIC
- published: 17 Oct 2011
- views: 11169
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron. Either iron(II) oxide (old term ferrous oxide, chemical formula FeO) or iron(III) oxide (old term ferric oxide, chemical formula Fe2O3). Generally known as rust when hydrated.. iron oxide synonyms: E172 when used as a food colouring. Iron oxide Meaning. How to pronounce, definition audio dictionary. How to say iron oxide. Powered by MaryTTS, Wiktionary
- published: 23 Apr 2015
- views: 236
This page is about a red-colored oxide of iron. For other uses, see red iron.
Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron(II) oxide (FeO), which is rare, and iron(II,III) oxide (Fe3O4), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is ferromagnetic, dark red, and readily attacked by acids. Iron(III) oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide.
This video is targeted to blind users.
Attribution:
Article text available under CC-BY-SA
Creative Commons image source in video
- published: 31 Aug 2014
- views: 676
Iron
Iron is a chemical element with symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal in the first transition series. It is by mass the most common element on Earth, forming much of Earth's outer and inner core. It is the fourth most common element in the Earth's crust. Its abundance in rocky planets like Earth is due to its abundant production by fusion in high-mass stars, where the production of nickel-56 (which decays to the most common isotope of iron) is the last nuclear fusion reaction that is exothermic. Consequently, radioactive nickel is the last element to be produced before the violent collapse of a supernova scatters precursor radionuclide of iron into space.
Like other group 8 elements, iron exists in a wide range of oxidation states, −2 to +6, although +2 and +3 are the most common. Elemental iron occurs in meteoroids and other low oxygen environments, but is reactive to oxygen and water. Fresh iron surfaces appear lustrous silvery-gray, but oxidize in normal air to give hydrated iron oxides, commonly known as rust. Unlike many other metals which form passivating oxide layers, iron oxides occupy more volume than the metal and thus flake off, exposing fresh surfaces for corrosion.
This page contains text from Wikipedia, the Free Encyclopedia -
http://wn.com/Iron
This article is licensed under the Creative Commons Attribution-ShareAlike 3.0 Unported License, which means that you can copy and modify it as long as the entire work (including additions) remains under this license.
This article is licensed under the Creative Commons Attribution-ShareAlike 3.0 Unported License, which means that you can copy and modify it as long as the entire work (including additions) remains under this license.
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2:36Iron(II) oxide
Iron(II) oxideIron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, which consists of hydrated iron(III) oxide (ferric oxide). Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O. This video is targeted to blind users. Attribution: Article text available under CC-BY-SA Creative Commons image source in video -
4:47DIY Iron(II) Oxide - Saline solution, concentration, and salt storage
DIY Iron(II) Oxide - Saline solution, concentration, and salt storageDIY Iron(II) Oxide - Saline solution, concentration, and salt storage
Full Details : http://dscript.org/homegrown-ironii-oxide This video demonstrates how to produce some home-grown Iron(II) Oxide, otherwise known as ferrous oxide, or black rust. Iron(II) Oxide is produced when Iron oxidises but does not have enough oxygen to get all the way up to Iron(III) Oxide. The oxidation process can be stalled and it will happily oxidise to black rust and stop there under the right conditions. The simplest way to do this is to put some iron in a sealed container. Fill it will heavily saturated salt water and let it sit for a few days. It helps if the iron is "pre-rusted" a bit to "jump start" the rusting process. The heavy concentration of salt will keep the levels of dissolved gases very low and deprive the iron of easy access to oxygen. As the iron rusts in low oxygen environment, it becomes Iron(II) Oxide and forms a layer of fine particulate on the bottom of the container. This stuff is used for many things, often as black colouring and dye. Concentrating it is a simple matter of using magnets, and at any point it can either be stored is it's salt water solution or dehydrated and bound to/into forming salt crystals. This is for DIY and experimental purposes only, please don't oxide iron or any other metals, excessively or unnecessarily, it takes alot of energy to reduce the original metal oxides into the pure metal form. every time you oxidise metals you are undoing alot of hard work. I plan to use this stuff in my water circuits. It will allow me to add magnetic responsivity into my fluid environment. Not sure if it will be used to "pump" water, open/close "gates" or various other applications. we will have to see what works ;) -
0:29Iron(II) oxide Meaning
Iron(II) oxide Meaning -
3:32Oxidation of Iron(II) to Iron(III) Using Potassium Manganate(VII)
Oxidation of Iron(II) to Iron(III) Using Potassium Manganate(VII) -
12:32Refining DIY Iron(II) Oxide - Round 2... Experiment!
Refining DIY Iron(II) Oxide - Round 2... Experiment!Refining DIY Iron(II) Oxide - Round 2... Experiment!
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage So I revisited the salt storage method for my ferrous oxide. I did a "harvest" on one of my production bottles and got a decent amount of ferrous oxide. so I decided to experiment. I figured there was enough for 3 good samples. The first I did a hard boil down of the salt-iron(II)oxide mixture - this produce a nice marble textured salt bed. On first glace it seems promising, the iron oxide is dispersed relatively well. For the second I added a bunch of vinegar - -
8:08Iron(II,III) oxide
Iron(II,III) oxideIron(II,III) oxide
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide, which is rare, and iron(III) oxide also known as hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic. Its most extensive use is as a black pigment which is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production. This video is targeted to blind users. Attribution: Article text available under CC-BY-SA Creative Commons image source in video -
63:12DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do organisms compete with chemical oxidation? ESD welcomes George W. Luther, Ph.D. (Univ. of Delaware) The oxidation of aqueous Fe(II) to Fe(III) solids is of great significance to Earth history including banded iron formation (BIFs) and the rise of O2 in waters and the atmosphere. The chemical oxidation of aqueous Fe(II) in air saturated solutions is facile at circumneutral pH, but O2 arises mainly from photosynthetic activity. There are currently three theories on how microbes could have contributed to Fe(III) precipitation: (1) oxygenic photosynthesis, coupled to abiotic Fe oxidation, (2) aerobic (anaerobic?) Fe oxidation by iron oxidizing bacteria (FeOB), and (3) anoxygenic photosynthesis, with Fe as an electron donor (photoferrotrophs). Using kinetic data obtained in the field as well as in the laboratory with in situ microelectrode techniques developed in our lab, it is now possible to discriminate between chemical Fe(II) oxidation and these microbially based processes in real time. Field data will be shown from diverse sites including Yellowstone National Park where groundwater, rich in Fe(II) and Mn(II) but with little or no O2, enter oxygenated systems. In the case of FeOB, their importance in Fe(II) oxidation increases at low O2 concentrations. Thermodynamic calculations for the first electron transfer between the metal ions, Fe(II) and Mn(II),with O2 over pH gives insight to the distribution of these metals in BIFs and their biogeochemical behavior. -
1:46REDOX : iron(II) sulfate oxidation with permanganate ion
REDOX : iron(II) sulfate oxidation with permanganate ionREDOX : iron(II) sulfate oxidation with permanganate ion
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following equation : 10 FeSO4 + 2 KMnO4 + 8 H2SO4 → 5 Fe2(SO4)3 + K2SO4 + 2 MnSO4 + 8 H2O Firs 98% sulfuric acid is added to 200 ml water in the Erlenmeyer flask and the two are mixed together. Then potassium permanganate solution is added. When the two are ready iron(II) sulfate solution is added to the flask causing an instantaneous change in color from the deep violet of permanganate ion to the light green - white of the iron(III) sulfate. This reaction is much faster than other because according to the collision theory only some collision are effective depending on the form of the molecule the temperature and the concentration . At the same concentration this reaction is much faster than other because of the nature of iron(II) ion that, being spherical, is reactive towards all oxidizing ions or molecules coming from all directions. WARNING IRON(II) SULFATE IS IRRITATING TOWARDS SKIN SULFURIC ACID IS CORROSIVE AND POTASSIUM PERMANGANATE IS HIGHLY TOXIC -
0:44Iron oxide Meaning
Iron oxide MeaningIron oxide Meaning
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron. Either iron(II) oxide (old term ferrous oxide, chemical formula FeO) or iron(III) oxide (old term ferric oxide, chemical formula Fe2O3). Generally known as rust when hydrated.. iron oxide synonyms: E172 when used as a food colouring. Iron oxide Meaning. How to pronounce, definition audio dictionary. How to say iron oxide. Powered by MaryTTS, Wiktionary -
9:41Iron(III) oxide
Iron(III) oxideIron(III) oxide
This page is about a red-colored oxide of iron. For other uses, see red iron. Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron(II) oxide (FeO), which is rare, and iron(II,III) oxide (Fe3O4), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is ferromagnetic, dark red, and readily attacked by acids. Iron(III) oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide. This video is targeted to blind users. Attribution: Article text available under CC-BY-SA Creative Commons image source in video
-
Iron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, which consists of hydrated iron(III) oxide (ferric oxide). Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O. This video is targeted to blind users. Attribution: Article text available under CC-BY-SA Creative Commons image source in video -
DIY Iron(II) Oxide - Saline solution, concentration, and salt storage
Full Details : http://dscript.org/homegrown-ironii-oxide This video demonstrates how to produce some home-grown Iron(II) Oxide, otherwise known as ferrous oxide, or black rust. Iron(II) Oxide is produced when Iron oxidises but does not have enough oxygen to get all the way up to Iron(III) Oxide. The oxidation process can be stalled and it will happily oxidise to black rust and stop there under the right conditions. The simplest way to do this is to put some iron in a sealed container. Fill it will heavily saturated salt water and let it sit for a few days. It helps if the iron is "pre-rusted" a bit to "jump start" the rusting process. The heavy concentration of salt will keep the levels of dissolved gases very low and deprive the iron of easy access to oxygen. As the iron rusts in low... -
-
-
Refining DIY Iron(II) Oxide - Round 2... Experiment!
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage So I revisited the salt storage method for my ferrous oxide. I did a "harvest" on one of my production bottles and got a decent amount of ferrous oxide. so I decided to experiment. I figured there was enough for 3 good samples. The first I did a hard boil down of the salt-iron(II)oxide mixture - this produce a nice marble textured salt bed. On first glace it seems promising, the iron oxide is dispersed relatively well. For the second I added a bunch of vinegar - -
Iron(II,III) oxide
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide, which is rare, and iron(III) oxide also known as hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic. Its most extensive use is as a black pigment which is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production. This video is targeted to blind users. Attribution: Article text available under CC-BY-SA Cre... -
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do organisms compete with chemical oxidation? ESD welcomes George W. Luther, Ph.D. (Univ. of Delaware) The oxidation of aqueous Fe(II) to Fe(III) solids is of great significance to Earth history including banded iron formation (BIFs) and the rise of O2 in waters and the atmosphere. The chemical oxidation of aqueous Fe(II) in air saturated solutions is facile at circumneutral pH, but O2 arises mainly from photosynthetic activity. There are currently three theories on how microbes could have contributed to Fe(III) precipitation: (1) oxygenic photosynthesis, coupled to abiotic Fe oxidation, (2) aerobic (anaerobic?) Fe oxidation by iron oxidizing bacteria (FeOB), and (3) anoxygenic photosynthesis, with Fe as ... -
REDOX : iron(II) sulfate oxidation with permanganate ion
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following equation : 10 FeSO4 + 2 KMnO4 + 8 H2SO4 → 5 Fe2(SO4)3 + K2SO4 + 2 MnSO4 + 8 H2O Firs 98% sulfuric acid is added to 200 ml water in the Erlenmeyer flask and the two are mixed together. Then potassium permanganate solution is added. When the two are ready iron(II) sulfate solution is added to the flask causing an instantaneous change in color from the deep violet of permanganate ion to the light green - white of the iron(III) sulfate. This reaction is much faster than other because according to the collision theory only some collision are effective depending on the form of the molecule the temperature and the concentration . At the same concentration this reaction is much faster than other because of t... -
Iron oxide Meaning
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron. Either iron(II) oxide (old term ferrous oxide, chemical formula FeO) or iron(III) oxide (old term ferric oxide, chemical formula Fe2O3). Generally known as rust when hydrated.. iron oxide synonyms: E172 when used as a food colouring. Iron oxide Meaning. How to pronounce, definition audio dictionary. How to say iron oxide. Powered by MaryTTS, Wiktionary -
Iron(III) oxide
This page is about a red-colored oxide of iron. For other uses, see red iron. Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron(II) oxide (FeO), which is rare, and iron(II,III) oxide (Fe3O4), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is ferromagnetic, dark red, and readily attacked by acids. Iron(III) oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide. This video is targeted to blind users. Attribution:...
Iron(II) oxide
- Order: Reorder
- Duration: 2:36
- Updated: 16 Nov 2014
- views: 433
Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder th...
Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, which consists of hydrated iron(III) oxide (ferric oxide). Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O.
This video is targeted to blind users.
Attribution:
Article text available under CC-BY-SA
Creative Commons image source in video
wn.com/Iron(Ii) Oxide
Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, which consists of hydrated iron(III) oxide (ferric oxide). Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O.
This video is targeted to blind users.
Attribution:
Article text available under CC-BY-SA
Creative Commons image source in video
- published: 16 Nov 2014
- views: 433
DIY Iron(II) Oxide - Saline solution, concentration, and salt storage
- Order: Reorder
- Duration: 4:47
- Updated: 15 Jul 2013
- views: 1359
Full Details : http://dscript.org/homegrown-ironii-oxide
This video demonstrates how to produce some home-grown Iron(II) Oxide, otherwise known as ferrous oxid...
Full Details : http://dscript.org/homegrown-ironii-oxide
This video demonstrates how to produce some home-grown Iron(II) Oxide, otherwise known as ferrous oxide, or black rust.
Iron(II) Oxide is produced when Iron oxidises but does not have enough oxygen to get all the way up to Iron(III) Oxide. The oxidation process can be stalled and it will happily oxidise to black rust and stop there under the right conditions.
The simplest way to do this is to put some iron in a sealed container. Fill it will heavily saturated salt water and let it sit for a few days. It helps if the iron is "pre-rusted" a bit to "jump start" the rusting process.
The heavy concentration of salt will keep the levels of dissolved gases very low and deprive the iron of easy access to oxygen.
As the iron rusts in low oxygen environment, it becomes Iron(II) Oxide and forms a layer of fine particulate on the bottom of the container.
This stuff is used for many things, often as black colouring and dye.
Concentrating it is a simple matter of using magnets, and at any point it can either be stored is it's salt water solution or dehydrated and bound to/into forming salt crystals.
This is for DIY and experimental purposes only, please don't oxide iron or any other metals, excessively or unnecessarily, it takes alot of energy to reduce the original metal oxides into the pure metal form. every time you oxidise metals you are undoing alot of hard work.
I plan to use this stuff in my water circuits. It will allow me to add magnetic responsivity into my fluid environment. Not sure if it will be used to "pump" water, open/close "gates" or various other applications. we will have to see what works ;)
wn.com/Diy Iron(Ii) Oxide Saline Solution, Concentration, And Salt Storage
Full Details : http://dscript.org/homegrown-ironii-oxide
This video demonstrates how to produce some home-grown Iron(II) Oxide, otherwise known as ferrous oxide, or black rust.
Iron(II) Oxide is produced when Iron oxidises but does not have enough oxygen to get all the way up to Iron(III) Oxide. The oxidation process can be stalled and it will happily oxidise to black rust and stop there under the right conditions.
The simplest way to do this is to put some iron in a sealed container. Fill it will heavily saturated salt water and let it sit for a few days. It helps if the iron is "pre-rusted" a bit to "jump start" the rusting process.
The heavy concentration of salt will keep the levels of dissolved gases very low and deprive the iron of easy access to oxygen.
As the iron rusts in low oxygen environment, it becomes Iron(II) Oxide and forms a layer of fine particulate on the bottom of the container.
This stuff is used for many things, often as black colouring and dye.
Concentrating it is a simple matter of using magnets, and at any point it can either be stored is it's salt water solution or dehydrated and bound to/into forming salt crystals.
This is for DIY and experimental purposes only, please don't oxide iron or any other metals, excessively or unnecessarily, it takes alot of energy to reduce the original metal oxides into the pure metal form. every time you oxidise metals you are undoing alot of hard work.
I plan to use this stuff in my water circuits. It will allow me to add magnetic responsivity into my fluid environment. Not sure if it will be used to "pump" water, open/close "gates" or various other applications. we will have to see what works ;)
- published: 15 Jul 2013
- views: 1359
Iron(II) oxide Meaning
- Order: Reorder
- Duration: 0:29
- Updated: 30 Apr 2015
- views: 93
Video shows what iron(II) oxide means. The chemical compound FeO, iron oxide where iron has a valence of +2.. Iron(II) oxide Meaning. How to pronounce, definit...
Video shows what iron(II) oxide means. The chemical compound FeO, iron oxide where iron has a valence of +2.. Iron(II) oxide Meaning. How to pronounce, definition audio dictionary. How to say iron(II) oxide. Powered by MaryTTS, Wiktionary
wn.com/Iron(Ii) Oxide Meaning
Oxidation of Iron(II) to Iron(III) Using Potassium Manganate(VII)
- Order: Reorder
- Duration: 3:32
- Updated: 16 Oct 2015
- views: 551
Oxidation of iron(II) ions to iron(III) ions in solution can be achieved through the addition of acidified potassium manganate(VII) solution.
Oxidation of iron(II) ions to iron(III) ions in solution can be achieved through the addition of acidified potassium manganate(VII) solution.
wn.com/Oxidation Of Iron(Ii) To Iron(Iii) Using Potassium Manganate(Vii)
Refining DIY Iron(II) Oxide - Round 2... Experiment!
- Order: Reorder
- Duration: 12:32
- Updated: 16 Jul 2013
- views: 625
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage
So I revisited the salt storage method for my ferrous oxide. I did a "harvest" on one o...
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage
So I revisited the salt storage method for my ferrous oxide. I did a "harvest" on one of my production bottles and got a decent amount of ferrous oxide. so I decided to experiment.
I figured there was enough for 3 good samples.
The first I did a hard boil down of the salt-iron(II)oxide mixture - this produce a nice marble textured salt bed. On first glace it seems promising, the iron oxide is dispersed relatively well.
For the second I added a bunch of vinegar -
wn.com/Refining Diy Iron(Ii) Oxide Round 2... Experiment
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage
So I revisited the salt storage method for my ferrous oxide. I did a "harvest" on one of my production bottles and got a decent amount of ferrous oxide. so I decided to experiment.
I figured there was enough for 3 good samples.
The first I did a hard boil down of the salt-iron(II)oxide mixture - this produce a nice marble textured salt bed. On first glace it seems promising, the iron oxide is dispersed relatively well.
For the second I added a bunch of vinegar -
- published: 16 Jul 2013
- views: 625
Iron(II,III) oxide
- Order: Reorder
- Duration: 8:08
- Updated: 22 Oct 2015
- views: 143
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others b...
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide, which is rare, and iron(III) oxide also known as hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic. Its most extensive use is as a black pigment which is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production.
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wn.com/Iron(Ii,Iii) Oxide
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide, which is rare, and iron(III) oxide also known as hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic. Its most extensive use is as a black pigment which is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production.
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- published: 22 Oct 2015
- views: 143
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
- Order: Reorder
- Duration: 63:12
- Updated: 05 Mar 2015
- views: 57
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do organisms compete with chemical oxidation?
ESD welcomes George W. Luthe...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do organisms compete with chemical oxidation?
ESD welcomes George W. Luther, Ph.D. (Univ. of Delaware)
The oxidation of aqueous Fe(II) to Fe(III) solids is of great significance to Earth history including banded iron formation (BIFs) and the rise of O2 in waters and the atmosphere. The chemical oxidation of aqueous Fe(II) in air saturated solutions is facile at circumneutral pH, but O2 arises mainly from photosynthetic activity. There are currently three theories on how microbes could have contributed to Fe(III) precipitation: (1) oxygenic photosynthesis, coupled to abiotic Fe oxidation, (2) aerobic (anaerobic?) Fe oxidation by iron oxidizing bacteria (FeOB), and (3) anoxygenic photosynthesis, with Fe as an electron donor (photoferrotrophs). Using kinetic data obtained in the field as well as in the laboratory with in situ microelectrode techniques developed in our lab, it is now possible to discriminate between chemical Fe(II) oxidation and these microbially based processes in real time. Field data will be shown from diverse sites including Yellowstone National Park where groundwater, rich in Fe(II) and Mn(II) but with little or no O2, enter oxygenated systems. In the case of FeOB, their importance in Fe(II) oxidation increases at low O2 concentrations. Thermodynamic calculations for the first electron transfer between the metal ions, Fe(II) and Mn(II),with O2 over pH gives insight to the distribution of these metals in BIFs and their biogeochemical behavior.
wn.com/Dsss Determining Chemical And Microbial Fe(Ii) Oxidation Kinetics In Situ...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do organisms compete with chemical oxidation?
ESD welcomes George W. Luther, Ph.D. (Univ. of Delaware)
The oxidation of aqueous Fe(II) to Fe(III) solids is of great significance to Earth history including banded iron formation (BIFs) and the rise of O2 in waters and the atmosphere. The chemical oxidation of aqueous Fe(II) in air saturated solutions is facile at circumneutral pH, but O2 arises mainly from photosynthetic activity. There are currently three theories on how microbes could have contributed to Fe(III) precipitation: (1) oxygenic photosynthesis, coupled to abiotic Fe oxidation, (2) aerobic (anaerobic?) Fe oxidation by iron oxidizing bacteria (FeOB), and (3) anoxygenic photosynthesis, with Fe as an electron donor (photoferrotrophs). Using kinetic data obtained in the field as well as in the laboratory with in situ microelectrode techniques developed in our lab, it is now possible to discriminate between chemical Fe(II) oxidation and these microbially based processes in real time. Field data will be shown from diverse sites including Yellowstone National Park where groundwater, rich in Fe(II) and Mn(II) but with little or no O2, enter oxygenated systems. In the case of FeOB, their importance in Fe(II) oxidation increases at low O2 concentrations. Thermodynamic calculations for the first electron transfer between the metal ions, Fe(II) and Mn(II),with O2 over pH gives insight to the distribution of these metals in BIFs and their biogeochemical behavior.
- published: 05 Mar 2015
- views: 57
REDOX : iron(II) sulfate oxidation with permanganate ion
- Order: Reorder
- Duration: 1:46
- Updated: 17 Oct 2011
- views: 11169
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following equation :
10 FeSO4 + 2 KMnO4 + 8 H2SO4 → 5 Fe2(SO4)3 + K2SO4 + 2 MnS...
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following equation :
10 FeSO4 + 2 KMnO4 + 8 H2SO4 → 5 Fe2(SO4)3 + K2SO4 + 2 MnSO4 + 8 H2O
Firs 98% sulfuric acid is added to 200 ml water in the Erlenmeyer flask and the two are mixed together.
Then potassium permanganate solution is added.
When the two are ready iron(II) sulfate solution is added to the flask causing an instantaneous change in color from the deep violet of permanganate ion to the light green - white of the iron(III) sulfate.
This reaction is much faster than other because according to the collision theory only some collision are effective depending on the form of the molecule the temperature and the concentration .
At the same concentration this reaction is much faster than other because of the nature of iron(II) ion that, being spherical, is reactive towards all oxidizing ions or molecules coming from all directions.
WARNING IRON(II) SULFATE IS IRRITATING TOWARDS SKIN SULFURIC ACID IS CORROSIVE AND POTASSIUM PERMANGANATE IS HIGHLY TOXIC
wn.com/Redox Iron(Ii) Sulfate Oxidation With Permanganate Ion
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following equation :
10 FeSO4 + 2 KMnO4 + 8 H2SO4 → 5 Fe2(SO4)3 + K2SO4 + 2 MnSO4 + 8 H2O
Firs 98% sulfuric acid is added to 200 ml water in the Erlenmeyer flask and the two are mixed together.
Then potassium permanganate solution is added.
When the two are ready iron(II) sulfate solution is added to the flask causing an instantaneous change in color from the deep violet of permanganate ion to the light green - white of the iron(III) sulfate.
This reaction is much faster than other because according to the collision theory only some collision are effective depending on the form of the molecule the temperature and the concentration .
At the same concentration this reaction is much faster than other because of the nature of iron(II) ion that, being spherical, is reactive towards all oxidizing ions or molecules coming from all directions.
WARNING IRON(II) SULFATE IS IRRITATING TOWARDS SKIN SULFURIC ACID IS CORROSIVE AND POTASSIUM PERMANGANATE IS HIGHLY TOXIC
- published: 17 Oct 2011
- views: 11169
Iron oxide Meaning
- Order: Reorder
- Duration: 0:44
- Updated: 23 Apr 2015
- views: 236
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron. Either iron(II) oxide (old term ferrous oxide, chemical formula FeO)...
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron. Either iron(II) oxide (old term ferrous oxide, chemical formula FeO) or iron(III) oxide (old term ferric oxide, chemical formula Fe2O3). Generally known as rust when hydrated.. iron oxide synonyms: E172 when used as a food colouring. Iron oxide Meaning. How to pronounce, definition audio dictionary. How to say iron oxide. Powered by MaryTTS, Wiktionary
wn.com/Iron Oxide Meaning
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron. Either iron(II) oxide (old term ferrous oxide, chemical formula FeO) or iron(III) oxide (old term ferric oxide, chemical formula Fe2O3). Generally known as rust when hydrated.. iron oxide synonyms: E172 when used as a food colouring. Iron oxide Meaning. How to pronounce, definition audio dictionary. How to say iron oxide. Powered by MaryTTS, Wiktionary
- published: 23 Apr 2015
- views: 236
Iron(III) oxide
- Order: Reorder
- Duration: 9:41
- Updated: 31 Aug 2014
- views: 676
This page is about a red-colored oxide of iron. For other uses, see red iron.
Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. ...
This page is about a red-colored oxide of iron. For other uses, see red iron.
Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron(II) oxide (FeO), which is rare, and iron(II,III) oxide (Fe3O4), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is ferromagnetic, dark red, and readily attacked by acids. Iron(III) oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide.
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wn.com/Iron(Iii) Oxide
This page is about a red-colored oxide of iron. For other uses, see red iron.
Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron(II) oxide (FeO), which is rare, and iron(II,III) oxide (Fe3O4), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is ferromagnetic, dark red, and readily attacked by acids. Iron(III) oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide.
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- published: 31 Aug 2014
- views: 676
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Iron(II) oxide
Iron(II) oxide Iron(II) oxide is the inorganic compound with the formula FeO.Its mineral form is known as wüstite. =======Image-Copyright-Info======= Image is in public domain Author-Info: http://en.wikipedia.org/w/index.php?title=User:Fuzic&action;=edit Image Source: https://en.wikipedia.org/wiki/File:Iron(II)_oxide.jpg =======Image-Copyright-Info======== -Video is targeted to blind users Attribution: Article text available under CC-BY-SA image source in video https://www.youtube.com/watch?v=hSVROOOIeEA -
Ferrous oxide Meaning
Video shows what ferrous oxide means. The chemical compound FeO, iron oxide where iron has a valence of +2. IUPAC has deprecated this term in favor of iron(II) oxide.. Ferrous oxide Meaning. How to pronounce, definition audio dictionary. How to say ferrous oxide. Powered by MaryTTS, Wiktionary
Iron(II) oxide
- Order: Reorder
- Duration: 2:32
- Updated: 22 Jan 2016
- views: 13
Iron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO.Its mineral form is known as wüstite.
=======Image-Copyright-Info=======
Image ...
Iron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO.Its mineral form is known as wüstite.
=======Image-Copyright-Info=======
Image is in public domain
Author-Info: http://en.wikipedia.org/w/index.php?title=User:Fuzic&action;=edit
Image Source: https://en.wikipedia.org/wiki/File:Iron(II)_oxide.jpg
=======Image-Copyright-Info========
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wn.com/Iron(Ii) Oxide
Iron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO.Its mineral form is known as wüstite.
=======Image-Copyright-Info=======
Image is in public domain
Author-Info: http://en.wikipedia.org/w/index.php?title=User:Fuzic&action;=edit
Image Source: https://en.wikipedia.org/wiki/File:Iron(II)_oxide.jpg
=======Image-Copyright-Info========
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- published: 22 Jan 2016
- views: 13
Ferrous oxide Meaning
- Order: Reorder
- Duration: 0:33
- Updated: 30 Apr 2015
- views: 58
Video shows what ferrous oxide means. The chemical compound FeO, iron oxide where iron has a valence of +2. IUPAC has deprecated this term in favor of iron(II) ...
Video shows what ferrous oxide means. The chemical compound FeO, iron oxide where iron has a valence of +2. IUPAC has deprecated this term in favor of iron(II) oxide.. Ferrous oxide Meaning. How to pronounce, definition audio dictionary. How to say ferrous oxide. Powered by MaryTTS, Wiktionary
wn.com/Ferrous Oxide Meaning
Video shows what ferrous oxide means. The chemical compound FeO, iron oxide where iron has a valence of +2. IUPAC has deprecated this term in favor of iron(II) oxide.. Ferrous oxide Meaning. How to pronounce, definition audio dictionary. How to say ferrous oxide. Powered by MaryTTS, Wiktionary
- published: 30 Apr 2015
- views: 58
-
Copper(II) oxide nanoparticles penetrate into HepG2 cells, exert cytotoxicity via oxidative stress
Jean‐Pascal Piret, University of Namur -
Iron
Iron is a chemical element with the symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal in the first transition series. It is by mass the most common element on Earth, forming much of Earth's outer and inner core. It is the fourth most common element in the Earth's crust. Iron's very common presence in rocky planets like Earth is due to its abundant production as a result of fusion in high-mass stars. Iron chemical compounds, which include ferrous and ferric compounds, have many uses. Iron oxide mixed with aluminium powder can be ignited to create a thermite reaction, used in welding and purifying ores. It forms binary compounds with the halogens and the chalcogens. Among its organometallic compounds is ferrocene, the first sandwich compound discovered. Iron plays an impor... -
The maufacturing of Aluminum
Aluminum isn't found in nature as a pure element. It exhibits relatively high chemical reactivity, which means it tends to bond with other elements to form compounds. More than 270 minerals in Earth's rocks and soils contain aluminum compounds. This makes aluminum the most abundant metal and the third most abundant element in Earth's crust. Only silicon and oxygen are more common than aluminum. The next most common metal after aluminum is iron, followed by magnesium, titanium and manganese. The primary source of aluminum is an ore known as bauxite. An ore is any naturally occurring solid material from which a metal or valuable mineral can be obtained. In this case, the solid material is a mixture of hydrated aluminum oxide and hydrated iron oxide. Hydrated refers to water molecules th... -
Inorganic Chemical Tests: Gases, Cations and Anions.
Flame Tests: Lithium – Crimson; Sodium – Yellow or Orange; Potassium - Lilac; Calcium - Brick red; Barium – Green; Copper - Green-blue or Blue-green. Tests for Gases: Hydrogen makes a pop with a lighted splint in air; Oxygen relights a glowing splint; Chlorine turns orange potassium dichromate solution green AND decolourises purple potassium permanganate; Ammonia forms a white smoke when a glass rod wet with concentrated hydrochloric acid is introduced. Hydrogen Chloride gas forms a white smoke when a glass rod wet with concentrated ammonia is introduced; Carbon Dioxide turns limewater cloudy; Sulfate ion solutions form a white precipitate with acidified barium chloride solution; Carbonates and Hydrogencarbonates produce effervescence (bubbles) when reacted with hydrochloric acid; Magnesiu... -
C1.3 Lesson2 Iron Extraction with Carbon
C1 AQA Extraction of iron, with some details about Blast furnace and reactions in blast furnace. Core Science AQA students do not need to know all the details but it is good for practicing balancing reactions. The core science students only need to know that iron oxide gets reduced to iron by heating with carbon and that is because carbon is more reactive than iron. -
Balancing Chemical Equations Tutorial - Examples & Practice Problems For Test / Exam Review
This video provides a tutorial on how to balance chemical equations such as combustion reactions, synthesis and decomposition reactions, single and double displacement reactions in addition to redox reactions under acidic and basic conditions. This video provides plenty of examples and practice problems that will help you to review for your next test or exam. Here is a list of equations covered in this video: 1. Combustion Reactions: Methane + oxygen gas yields carbon dioxide and water OR CH4 + O2 = CO2 + H2O Propane: C3H8 + O2 = CO2 + H2O Ethane: C2H6 + O2 = CO2 + H2O Ethanol: C2H5OH + O2 = CO2 + H2O Propanol: C3H7OH + O2 = CO2 + H2O Benzene: C6H6 + O2 = CO2 + H2O 2. Balancing Synthesis & Decomposition Reactions N2 + H2 = NH3 (nitrogen gas + oxygen gas yields ammonia) S8 + O2 = SO3 (s... -
Reversible Reactions
Reversible Reactions: In this lesson we will study reversible reactions. In the above chemical reactions the first positive sign means react with and the second on the product side means 'and' The arrow shows the direction to which the reaction proceeds . Therefore the whole chemical change is represented as; Fe (s) + 2HCl(aq) w FeCl 2 (aq) + H 2 (g) In the second example the reactants are sulphur and Oxygen while the products is Sulphur (IV) oxide since Oxygen gas is limited not excess. The reaction should be presented as S (s) + O2 (g) w SO2(g) Reversible reaction is a chemical reaction in which the products of forward reaction can combine to give back the original reactants. Iron reacts with water to form Iron (III) oxide and hydrogen gas. In the reaction the double arrow means rever... -
Mod-03 Lec-19 Metal and Metal Oxide Nanowires - II
Nano structured materials-synthesis, properties, self assembly and applications by Prof. A.K. Ganguli,Department of Nanotechnology,IIT Delhi.For more details on NPTEL visit http://nptel.ac.in -
Super Metroid Oxide (Stream)
So yeah. . . I decided to stream Oxide for fun. This hack still holds up to the goofiness I remember from it. Definitely worth your time to play. [Hack Page] http://metroidconstruction.com/hacks.php?h=h95 [Facebook] https://www.facebook.com/ShyGuyExpress [Twitter] https://twitter.com/MetroidMst [YouTube Channel] http://www.youtube.com/user/ShyGuyExpress [Stream Channel] http://www.hitbox.tv/MetroidMst
Copper(II) oxide nanoparticles penetrate into HepG2 cells, exert cytotoxicity via oxidative stress
- Order: Reorder
- Duration: 21:04
- Updated: 07 Apr 2013
- views: 203
Jean‐Pascal Piret, University of Namur
Jean‐Pascal Piret, University of Namur
wn.com/Copper(Ii) Oxide Nanoparticles Penetrate Into Hepg2 Cells, Exert Cytotoxicity Via Oxidative Stress
Iron
- Order: Reorder
- Duration: 43:37
- Updated: 20 May 2014
- views: 260656
Iron is a chemical element with the symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal in the first transition series. It is by mass the most co...
Iron is a chemical element with the symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal in the first transition series. It is by mass the most common element on Earth, forming much of Earth's outer and inner core. It is the fourth most common element in the Earth's crust. Iron's very common presence in rocky planets like Earth is due to its abundant production as a result of fusion in high-mass stars.
Iron chemical compounds, which include ferrous and ferric compounds, have many uses. Iron oxide mixed with aluminium powder can be ignited to create a thermite reaction, used in welding and purifying ores. It forms binary compounds with the halogens and the chalcogens. Among its organometallic compounds is ferrocene, the first sandwich compound discovered.
Iron plays an important role in biology, forming complexes with molecular oxygen in hemoglobin and myoglobin; these two compounds are common oxygen transport proteins in vertebrates. Iron is also the metal used at the active site of many important redox enzymes dealing with cellular respiration and oxidation and reduction in plants and animals.
wn.com/Iron
Iron is a chemical element with the symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal in the first transition series. It is by mass the most common element on Earth, forming much of Earth's outer and inner core. It is the fourth most common element in the Earth's crust. Iron's very common presence in rocky planets like Earth is due to its abundant production as a result of fusion in high-mass stars.
Iron chemical compounds, which include ferrous and ferric compounds, have many uses. Iron oxide mixed with aluminium powder can be ignited to create a thermite reaction, used in welding and purifying ores. It forms binary compounds with the halogens and the chalcogens. Among its organometallic compounds is ferrocene, the first sandwich compound discovered.
Iron plays an important role in biology, forming complexes with molecular oxygen in hemoglobin and myoglobin; these two compounds are common oxygen transport proteins in vertebrates. Iron is also the metal used at the active site of many important redox enzymes dealing with cellular respiration and oxidation and reduction in plants and animals.
- published: 20 May 2014
- views: 260656
The maufacturing of Aluminum
- Order: Reorder
- Duration: 41:43
- Updated: 24 Mar 2016
- views: 154
Aluminum isn't found in nature as a pure element. It exhibits relatively high chemical reactivity, which means it tends to bond with other elements to form comp...
Aluminum isn't found in nature as a pure element. It exhibits relatively high chemical reactivity, which means it tends to bond with other elements to form compounds. More than 270 minerals in Earth's rocks and soils contain aluminum compounds. This makes aluminum the most abundant metal and the third most abundant element in Earth's crust. Only silicon and oxygen are more common than aluminum. The next most common metal after aluminum is iron, followed by magnesium, titanium and manganese.
The primary source of aluminum is an ore known as bauxite. An ore is any naturally occurring solid material from which a metal or valuable mineral can be obtained. In this case, the solid material is a mixture of hydrated aluminum oxide and hydrated iron oxide. Hydrated refers to water molecules that are chemically bound to the two compounds. The chemical formula for aluminum oxide is Al2O3. The formula for iron oxide is Fe2O3.
Deposits of bauxite occur as flat layers lying near the Earth's surface and may cover many miles. Geologists locate these deposits by prospecting -- taking core samples or drilling in soils suspected of containing the ore. By analyzing the cores, scientists are able to determine the quantity and quality of the bauxite.
After the ore is discovered, open-pit mines typically provide the bauxite that will eventually become aluminum. First bulldozers clear land above a deposit. Then workers loosen the soil with explosives, which bring the ore to the surface. Giant shovels then scoop up the bauxite-rich soil and dump it into trucks, which carry the ore to a processing plant. France was the first site of large-scale bauxite mining. In the United States, Arkansas was a major supplier of bauxite before, during and after World War II. But today, the material is predominantly mined in Australia, Africa, South America and the Caribbean.
The first step in the commercial production of aluminum is the separation of aluminum oxide from the iron oxide in bauxite. This is accomplished using a technique developed by Karl Joseph Bayer, an Austrian chemist, in 1888. In the Bayer process, bauxite is mixed with caustic soda, or sodium hydroxide, and heated under pressure. The sodium hydroxide dissolves the aluminum oxide, forming sodium aluminate. The iron oxide remains solid and is separated by filtration. Finally, aluminum hydroxide introduced to the liquid sodium aluminate causes aluminum oxide to precipitate, or come out of solution as a solid. These crystals are washed and heated to get rid of the water. The result is pure aluminum oxide, a fine white powder also known as alumina.
Alumina is a handy material in its own right. Its hardness makes it useful as an abrasive and as a component in cutting tools. It can also be used to purify water and to make ceramics and other building materials. But its primary use is to act as a starting point to extract pure aluminum. In the next section, we'll see look at the steps required to transform alumina into aluminum.
wn.com/The Maufacturing Of Aluminum
Aluminum isn't found in nature as a pure element. It exhibits relatively high chemical reactivity, which means it tends to bond with other elements to form compounds. More than 270 minerals in Earth's rocks and soils contain aluminum compounds. This makes aluminum the most abundant metal and the third most abundant element in Earth's crust. Only silicon and oxygen are more common than aluminum. The next most common metal after aluminum is iron, followed by magnesium, titanium and manganese.
The primary source of aluminum is an ore known as bauxite. An ore is any naturally occurring solid material from which a metal or valuable mineral can be obtained. In this case, the solid material is a mixture of hydrated aluminum oxide and hydrated iron oxide. Hydrated refers to water molecules that are chemically bound to the two compounds. The chemical formula for aluminum oxide is Al2O3. The formula for iron oxide is Fe2O3.
Deposits of bauxite occur as flat layers lying near the Earth's surface and may cover many miles. Geologists locate these deposits by prospecting -- taking core samples or drilling in soils suspected of containing the ore. By analyzing the cores, scientists are able to determine the quantity and quality of the bauxite.
After the ore is discovered, open-pit mines typically provide the bauxite that will eventually become aluminum. First bulldozers clear land above a deposit. Then workers loosen the soil with explosives, which bring the ore to the surface. Giant shovels then scoop up the bauxite-rich soil and dump it into trucks, which carry the ore to a processing plant. France was the first site of large-scale bauxite mining. In the United States, Arkansas was a major supplier of bauxite before, during and after World War II. But today, the material is predominantly mined in Australia, Africa, South America and the Caribbean.
The first step in the commercial production of aluminum is the separation of aluminum oxide from the iron oxide in bauxite. This is accomplished using a technique developed by Karl Joseph Bayer, an Austrian chemist, in 1888. In the Bayer process, bauxite is mixed with caustic soda, or sodium hydroxide, and heated under pressure. The sodium hydroxide dissolves the aluminum oxide, forming sodium aluminate. The iron oxide remains solid and is separated by filtration. Finally, aluminum hydroxide introduced to the liquid sodium aluminate causes aluminum oxide to precipitate, or come out of solution as a solid. These crystals are washed and heated to get rid of the water. The result is pure aluminum oxide, a fine white powder also known as alumina.
Alumina is a handy material in its own right. Its hardness makes it useful as an abrasive and as a component in cutting tools. It can also be used to purify water and to make ceramics and other building materials. But its primary use is to act as a starting point to extract pure aluminum. In the next section, we'll see look at the steps required to transform alumina into aluminum.
- published: 24 Mar 2016
- views: 154
Inorganic Chemical Tests: Gases, Cations and Anions.
- Order: Reorder
- Duration: 28:41
- Updated: 24 Apr 2016
- views: 1048
Flame Tests: Lithium – Crimson; Sodium – Yellow or Orange; Potassium - Lilac; Calcium - Brick red; Barium – Green; Copper - Green-blue or Blue-green. Tests for ...
Flame Tests: Lithium – Crimson; Sodium – Yellow or Orange; Potassium - Lilac; Calcium - Brick red; Barium – Green; Copper - Green-blue or Blue-green. Tests for Gases: Hydrogen makes a pop with a lighted splint in air; Oxygen relights a glowing splint; Chlorine turns orange potassium dichromate solution green AND decolourises purple potassium permanganate; Ammonia forms a white smoke when a glass rod wet with concentrated hydrochloric acid is introduced. Hydrogen Chloride gas forms a white smoke when a glass rod wet with concentrated ammonia is introduced; Carbon Dioxide turns limewater cloudy; Sulfate ion solutions form a white precipitate with acidified barium chloride solution; Carbonates and Hydrogencarbonates produce effervescence (bubbles) when reacted with hydrochloric acid; Magnesium ions in solution can be used to distinguish between carbonate and hydrogencarbonate solutions (forming a precipitate with the carbonate only); Halide ions (Chloride, Bromide and Iodide) in aqueous solution can be identified using acidified silver nitrate solution – following a test with dilute and concentrated ammonia solution to see if the silver halide precipitates can be re-dissolved; Barium ion in solution using potassium chromate solution, followed by dilute hydrochloric acid; Copper (II) ions in solution with an ammonia solution added in a dropwise fashion until in excess; Ammonium ions in a salt by warming with sodium hydroxide and testing for the evolution of ammonia gas using a glass rod wet with concentrated hydrochloric acid; Iron (II) and Iron (III) salt solutions with dilute sodium hydroxide solution; Magnesium, aluminium and Zinc (II) salt solutions distinguished by first reacting with aqueous sodium hydroxide and then with aqueous ammonia solutions; Iron (III) salt solutions with aqueous potassium thiocyanate. Essentially, this matches CCEA's excellent handout called "Acceptable Colour Changes".
wn.com/Inorganic Chemical Tests Gases, Cations And Anions.
Flame Tests: Lithium – Crimson; Sodium – Yellow or Orange; Potassium - Lilac; Calcium - Brick red; Barium – Green; Copper - Green-blue or Blue-green. Tests for Gases: Hydrogen makes a pop with a lighted splint in air; Oxygen relights a glowing splint; Chlorine turns orange potassium dichromate solution green AND decolourises purple potassium permanganate; Ammonia forms a white smoke when a glass rod wet with concentrated hydrochloric acid is introduced. Hydrogen Chloride gas forms a white smoke when a glass rod wet with concentrated ammonia is introduced; Carbon Dioxide turns limewater cloudy; Sulfate ion solutions form a white precipitate with acidified barium chloride solution; Carbonates and Hydrogencarbonates produce effervescence (bubbles) when reacted with hydrochloric acid; Magnesium ions in solution can be used to distinguish between carbonate and hydrogencarbonate solutions (forming a precipitate with the carbonate only); Halide ions (Chloride, Bromide and Iodide) in aqueous solution can be identified using acidified silver nitrate solution – following a test with dilute and concentrated ammonia solution to see if the silver halide precipitates can be re-dissolved; Barium ion in solution using potassium chromate solution, followed by dilute hydrochloric acid; Copper (II) ions in solution with an ammonia solution added in a dropwise fashion until in excess; Ammonium ions in a salt by warming with sodium hydroxide and testing for the evolution of ammonia gas using a glass rod wet with concentrated hydrochloric acid; Iron (II) and Iron (III) salt solutions with dilute sodium hydroxide solution; Magnesium, aluminium and Zinc (II) salt solutions distinguished by first reacting with aqueous sodium hydroxide and then with aqueous ammonia solutions; Iron (III) salt solutions with aqueous potassium thiocyanate. Essentially, this matches CCEA's excellent handout called "Acceptable Colour Changes".
- published: 24 Apr 2016
- views: 1048
C1.3 Lesson2 Iron Extraction with Carbon
- Order: Reorder
- Duration: 27:22
- Updated: 16 Feb 2015
- views: 410
C1 AQA Extraction of iron, with some details about Blast furnace and reactions in blast furnace. Core Science AQA students do not need to know all the details b...
C1 AQA Extraction of iron, with some details about Blast furnace and reactions in blast furnace. Core Science AQA students do not need to know all the details but it is good for practicing balancing reactions. The core science students only need to know that iron oxide gets reduced to iron by heating with carbon and that is because carbon is more reactive than iron.
wn.com/C1.3 Lesson2 Iron Extraction With Carbon
C1 AQA Extraction of iron, with some details about Blast furnace and reactions in blast furnace. Core Science AQA students do not need to know all the details but it is good for practicing balancing reactions. The core science students only need to know that iron oxide gets reduced to iron by heating with carbon and that is because carbon is more reactive than iron.
- published: 16 Feb 2015
- views: 410
Balancing Chemical Equations Tutorial - Examples & Practice Problems For Test / Exam Review
- Order: Reorder
- Duration: 31:49
- Updated: 14 Feb 2016
- views: 1207
This video provides a tutorial on how to balance chemical equations such as combustion reactions, synthesis and decomposition reactions, single and double displ...
This video provides a tutorial on how to balance chemical equations such as combustion reactions, synthesis and decomposition reactions, single and double displacement reactions in addition to redox reactions under acidic and basic conditions. This video provides plenty of examples and practice problems that will help you to review for your next test or exam.
Here is a list of equations covered in this video:
1. Combustion Reactions:
Methane + oxygen gas yields carbon dioxide and water OR
CH4 + O2 = CO2 + H2O
Propane: C3H8 + O2 = CO2 + H2O
Ethane: C2H6 + O2 = CO2 + H2O
Ethanol: C2H5OH + O2 = CO2 + H2O
Propanol: C3H7OH + O2 = CO2 + H2O
Benzene: C6H6 + O2 = CO2 + H2O
2. Balancing Synthesis & Decomposition Reactions
N2 + H2 = NH3 (nitrogen gas + oxygen gas yields ammonia)
S8 + O2 = SO3 (sulfur + oxygen gas yields sulfur trioxide)
P4 + Cl2 = PCl3 (phosphorus + chlorine gas yields phosphorus trichloride)
Al(OH)3 + CO2 = Al(HCO3)3 (aluminum hydroxide and carbon dioxide gas yields aluminum bicarbonate)
KClO3 = KCl + O2 (potassium chlorate yields potassium chloride and oxygen gas)
Mg3N2 = Mg + N2 (magnesium nitride yields magnesium and nitrogen gas)
3. Al + CuSO4 = Al2(SO4)3 + Cu (aluminum metal and aqueous copper ii sulfate yields aluminum sulfate and copper metal)
K + FeCl2 = KCl + Fe (potassium metal and iron ii chloride yields aqueous potassium chlorine and iron metal)
Na2S + Cl2 = NaCl + S8 (sodium sulfide reacts with chlorine gas to produce sodium chloride and elemental sulfur)
4. How To Balance Double Replacement Reactions:
NaCl + Pb(NO3)2 = PbCl2 + NaNO3
Aqueous sodium chloride reacts with lead (II) nitrate to produce lead (II) chloride and aqueous sodium nitrate
ZnBr2 + Na3PO4 = Zn3(PO4)2 + NaBr
Zinc bromide reacts with sodium phosphate to produce solid zinc phosphate and sodium bromide
Sn(NO3)4 + K3PO3 = Sn3(PO3)4 + KNO3
Tin (IV) Nitrate and potassium phosphite reacts to produce solid tin (IV) phosphite and potassium nitrate
Balancing Redox Reactions In Acidic, Basic, and Neutral Solutions:
Al + Ni2+ = Ni + Al3+
Zn + ClO- = Cl- + Zn2+ (acidic conditions)
Al + BrO4- = Br- + Al3+ (basic conditions)
wn.com/Balancing Chemical Equations Tutorial Examples Practice Problems For Test Exam Review
This video provides a tutorial on how to balance chemical equations such as combustion reactions, synthesis and decomposition reactions, single and double displacement reactions in addition to redox reactions under acidic and basic conditions. This video provides plenty of examples and practice problems that will help you to review for your next test or exam.
Here is a list of equations covered in this video:
1. Combustion Reactions:
Methane + oxygen gas yields carbon dioxide and water OR
CH4 + O2 = CO2 + H2O
Propane: C3H8 + O2 = CO2 + H2O
Ethane: C2H6 + O2 = CO2 + H2O
Ethanol: C2H5OH + O2 = CO2 + H2O
Propanol: C3H7OH + O2 = CO2 + H2O
Benzene: C6H6 + O2 = CO2 + H2O
2. Balancing Synthesis & Decomposition Reactions
N2 + H2 = NH3 (nitrogen gas + oxygen gas yields ammonia)
S8 + O2 = SO3 (sulfur + oxygen gas yields sulfur trioxide)
P4 + Cl2 = PCl3 (phosphorus + chlorine gas yields phosphorus trichloride)
Al(OH)3 + CO2 = Al(HCO3)3 (aluminum hydroxide and carbon dioxide gas yields aluminum bicarbonate)
KClO3 = KCl + O2 (potassium chlorate yields potassium chloride and oxygen gas)
Mg3N2 = Mg + N2 (magnesium nitride yields magnesium and nitrogen gas)
3. Al + CuSO4 = Al2(SO4)3 + Cu (aluminum metal and aqueous copper ii sulfate yields aluminum sulfate and copper metal)
K + FeCl2 = KCl + Fe (potassium metal and iron ii chloride yields aqueous potassium chlorine and iron metal)
Na2S + Cl2 = NaCl + S8 (sodium sulfide reacts with chlorine gas to produce sodium chloride and elemental sulfur)
4. How To Balance Double Replacement Reactions:
NaCl + Pb(NO3)2 = PbCl2 + NaNO3
Aqueous sodium chloride reacts with lead (II) nitrate to produce lead (II) chloride and aqueous sodium nitrate
ZnBr2 + Na3PO4 = Zn3(PO4)2 + NaBr
Zinc bromide reacts with sodium phosphate to produce solid zinc phosphate and sodium bromide
Sn(NO3)4 + K3PO3 = Sn3(PO3)4 + KNO3
Tin (IV) Nitrate and potassium phosphite reacts to produce solid tin (IV) phosphite and potassium nitrate
Balancing Redox Reactions In Acidic, Basic, and Neutral Solutions:
Al + Ni2+ = Ni + Al3+
Zn + ClO- = Cl- + Zn2+ (acidic conditions)
Al + BrO4- = Br- + Al3+ (basic conditions)
- published: 14 Feb 2016
- views: 1207
Reversible Reactions
- Order: Reorder
- Duration: 20:41
- Updated: 29 Oct 2015
- views: 228
Reversible Reactions: In this lesson we will study reversible reactions.
In the above chemical reactions the first positive sign means react with and the secon...
Reversible Reactions: In this lesson we will study reversible reactions.
In the above chemical reactions the first positive sign means react with and the second on the product side means 'and'
The arrow shows the direction to which the reaction proceeds . Therefore the whole chemical change is represented as;
Fe (s) + 2HCl(aq) w FeCl 2 (aq) + H 2 (g)
In the second example the reactants are sulphur and Oxygen while the products is Sulphur (IV) oxide since Oxygen gas is limited not excess. The reaction should be presented as
S (s) + O2 (g) w SO2(g)
Reversible reaction is a chemical reaction in which the products of forward reaction can combine to give back the original reactants.
Iron reacts with water to form Iron (III) oxide and hydrogen gas.
In the reaction the double arrow means reversible so that rate of forward and backward reactions are the same.
Forward reaction has Iron and steam as the reactants and tri Iron tetra Oxide and hydrogen as products.
Backward reaction has tri Iron tetra oxide and hydrogen as reactants and Iron and steam as products.
Calcium carbonate decomposes to Calcium oxide and carbon (IV) oxide gas.
In the equation when the reaction takes place in a closed system initially it decomposes to form lime (Calcium oxide) and Carbon (IV) oxide. This is the forward reaction.Backward reaction is favoured by accumulation of Carbon (IV) oxide that reacts with lime to form limestone (Calcium Carbonate)
which is given off and a white solid is left behind.
Hydrated Copper (II) crystals lose water of crystallization as shown in the following equation.
When blue crystals of Copper (II) Sulphate are heated in a test tube steam is given off and a white solid is left behind.
When the tube is cooled and a few drops of cold water added the blue colour reappears and the tube becomes hot.
The following experiment is carried out to investigate the chemical equilibrium in Chromate (VI) ion. Click to play the video and observe what happens carefully.
Potassium chromate (VI) solution is orange. When a few drops of dilute hydrochloric acid are added to the solution it turns yellow due to the formation of dichromate (VI) ions (Cr 2 O7 2-). This makes the concentration of hydrogen ions to increase as the acid is added.
An equilibrium is established with more Cr 2 O7 2- in solution than Cr O42- hence orange colour is dorminant.
On adding a few drops of 2M Sodium hydroxide the colour of the solution turns to orange as shown in the equation.
On adding 2M sodium hydroxide OH- ions react with H+ ions to form water. This reduces concentration of H+ ions in the solution shifting the equilibrium to the left.
H+ ions are formed to replace the H+ ions used to form water.
Altering the concentration of any one of the components of the equilibrium mixture disturbs equilibrium by affecting the rate of forward and backward reaction.
This makes the reaction proceed in one direction until a new equilibrium is established.
Note that the arrow showing reversible at equilibrium as shown
Which is different to that of the normal reversible reaction.
When the rate of forward reaction equals the rate of backward reaction a state of balance is reached.
At first D and C dominates to form F and G and then as F and G accumulates reverse reaction starts building up until a state of balance is reached.
At the state of balance the reaction is said to have reached a dynamic equilibrium because reactants and products are simply co existing but there is constant interchange from products to reactants and vice versa.
The following experiment explains chemical equilibrium as a state of balance.
The video clip below shows how to investigate change of colour of indicator in acid alkali media as an example of reversible reactions.Click to play the video and observe what happens carefully.
Phenolphthalein indicator is colourless in water and acid.
It is pink in alkali
In reversible reactions products can form reactants unlike many reactions that are one way.
In a closed system where no reactants or products escape both forward and backward reactions occur at the same time.
As time goes both forward and backward reactions proceed at the same rate. This is called chemical Equilibrium or dynamic equilibrium. The individual atoms and molecules reacting and products do not change in concentration.
You will now learn about the factors affecting rates of reaction.
wn.com/Reversible Reactions
Reversible Reactions: In this lesson we will study reversible reactions.
In the above chemical reactions the first positive sign means react with and the second on the product side means 'and'
The arrow shows the direction to which the reaction proceeds . Therefore the whole chemical change is represented as;
Fe (s) + 2HCl(aq) w FeCl 2 (aq) + H 2 (g)
In the second example the reactants are sulphur and Oxygen while the products is Sulphur (IV) oxide since Oxygen gas is limited not excess. The reaction should be presented as
S (s) + O2 (g) w SO2(g)
Reversible reaction is a chemical reaction in which the products of forward reaction can combine to give back the original reactants.
Iron reacts with water to form Iron (III) oxide and hydrogen gas.
In the reaction the double arrow means reversible so that rate of forward and backward reactions are the same.
Forward reaction has Iron and steam as the reactants and tri Iron tetra Oxide and hydrogen as products.
Backward reaction has tri Iron tetra oxide and hydrogen as reactants and Iron and steam as products.
Calcium carbonate decomposes to Calcium oxide and carbon (IV) oxide gas.
In the equation when the reaction takes place in a closed system initially it decomposes to form lime (Calcium oxide) and Carbon (IV) oxide. This is the forward reaction.Backward reaction is favoured by accumulation of Carbon (IV) oxide that reacts with lime to form limestone (Calcium Carbonate)
which is given off and a white solid is left behind.
Hydrated Copper (II) crystals lose water of crystallization as shown in the following equation.
When blue crystals of Copper (II) Sulphate are heated in a test tube steam is given off and a white solid is left behind.
When the tube is cooled and a few drops of cold water added the blue colour reappears and the tube becomes hot.
The following experiment is carried out to investigate the chemical equilibrium in Chromate (VI) ion. Click to play the video and observe what happens carefully.
Potassium chromate (VI) solution is orange. When a few drops of dilute hydrochloric acid are added to the solution it turns yellow due to the formation of dichromate (VI) ions (Cr 2 O7 2-). This makes the concentration of hydrogen ions to increase as the acid is added.
An equilibrium is established with more Cr 2 O7 2- in solution than Cr O42- hence orange colour is dorminant.
On adding a few drops of 2M Sodium hydroxide the colour of the solution turns to orange as shown in the equation.
On adding 2M sodium hydroxide OH- ions react with H+ ions to form water. This reduces concentration of H+ ions in the solution shifting the equilibrium to the left.
H+ ions are formed to replace the H+ ions used to form water.
Altering the concentration of any one of the components of the equilibrium mixture disturbs equilibrium by affecting the rate of forward and backward reaction.
This makes the reaction proceed in one direction until a new equilibrium is established.
Note that the arrow showing reversible at equilibrium as shown
Which is different to that of the normal reversible reaction.
When the rate of forward reaction equals the rate of backward reaction a state of balance is reached.
At first D and C dominates to form F and G and then as F and G accumulates reverse reaction starts building up until a state of balance is reached.
At the state of balance the reaction is said to have reached a dynamic equilibrium because reactants and products are simply co existing but there is constant interchange from products to reactants and vice versa.
The following experiment explains chemical equilibrium as a state of balance.
The video clip below shows how to investigate change of colour of indicator in acid alkali media as an example of reversible reactions.Click to play the video and observe what happens carefully.
Phenolphthalein indicator is colourless in water and acid.
It is pink in alkali
In reversible reactions products can form reactants unlike many reactions that are one way.
In a closed system where no reactants or products escape both forward and backward reactions occur at the same time.
As time goes both forward and backward reactions proceed at the same rate. This is called chemical Equilibrium or dynamic equilibrium. The individual atoms and molecules reacting and products do not change in concentration.
You will now learn about the factors affecting rates of reaction.
- published: 29 Oct 2015
- views: 228
Mod-03 Lec-19 Metal and Metal Oxide Nanowires - II
- Order: Reorder
- Duration: 57:07
- Updated: 02 Sep 2014
- views: 563
Nano structured materials-synthesis, properties, self assembly and applications by Prof. A.K. Ganguli,Department of Nanotechnology,IIT Delhi.For more details on...
Nano structured materials-synthesis, properties, self assembly and applications by Prof. A.K. Ganguli,Department of Nanotechnology,IIT Delhi.For more details on NPTEL visit http://nptel.ac.in
wn.com/Mod 03 Lec 19 Metal And Metal Oxide Nanowires Ii
Nano structured materials-synthesis, properties, self assembly and applications by Prof. A.K. Ganguli,Department of Nanotechnology,IIT Delhi.For more details on NPTEL visit http://nptel.ac.in
- published: 02 Sep 2014
- views: 563
Super Metroid Oxide (Stream)
- Order: Reorder
- Duration: 115:39
- Updated: 11 Aug 2014
- views: 1706
So yeah. . . I decided to stream Oxide for fun. This hack still holds up to the goofiness I remember from it. Definitely worth your time to play.
[Hack Page] h...
So yeah. . . I decided to stream Oxide for fun. This hack still holds up to the goofiness I remember from it. Definitely worth your time to play.
[Hack Page] http://metroidconstruction.com/hacks.php?h=h95
[Facebook] https://www.facebook.com/ShyGuyExpress
[Twitter] https://twitter.com/MetroidMst
[YouTube Channel] http://www.youtube.com/user/ShyGuyExpress
[Stream Channel] http://www.hitbox.tv/MetroidMst
wn.com/Super Metroid Oxide (Stream)
So yeah. . . I decided to stream Oxide for fun. This hack still holds up to the goofiness I remember from it. Definitely worth your time to play.
[Hack Page] http://metroidconstruction.com/hacks.php?h=h95
[Facebook] https://www.facebook.com/ShyGuyExpress
[Twitter] https://twitter.com/MetroidMst
[YouTube Channel] http://www.youtube.com/user/ShyGuyExpress
[Stream Channel] http://www.hitbox.tv/MetroidMst
- published: 11 Aug 2014
- views: 1706
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2:36
Iron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known a...
published: 16 Nov 2014
Iron(II) oxide
Iron(II) oxide
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- published: 16 Nov 2014
- views: 433
4:47
DIY Iron(II) Oxide - Saline solution, concentration, and salt storage
Full Details : http://dscript.org/homegrown-ironii-oxide
This video demonstrates how to p...
published: 15 Jul 2013
DIY Iron(II) Oxide - Saline solution, concentration, and salt storage
DIY Iron(II) Oxide - Saline solution, concentration, and salt storage
- Report rights infringement
- published: 15 Jul 2013
- views: 1359
0:29
Iron(II) oxide Meaning
Video shows what iron(II) oxide means. The chemical compound FeO, iron oxide where iron ha...
published: 30 Apr 2015
Iron(II) oxide Meaning
Iron(II) oxide Meaning
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- published: 30 Apr 2015
- views: 93
3:32
Oxidation of Iron(II) to Iron(III) Using Potassium Manganate(VII)
Oxidation of iron(II) ions to iron(III) ions in solution can be achieved through the addit...
published: 16 Oct 2015
Oxidation of Iron(II) to Iron(III) Using Potassium Manganate(VII)
Oxidation of Iron(II) to Iron(III) Using Potassium Manganate(VII)
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- published: 16 Oct 2015
- views: 551
12:32
Refining DIY Iron(II) Oxide - Round 2... Experiment!
Full Details: http://dscript.org/ironii-oxide-diy-production-and-storage
So I revisited th...
published: 16 Jul 2013
Refining DIY Iron(II) Oxide - Round 2... Experiment!
Refining DIY Iron(II) Oxide - Round 2... Experiment!
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- published: 16 Jul 2013
- views: 625
8:08
Iron(II,III) oxide
Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the...
published: 22 Oct 2015
Iron(II,III) oxide
Iron(II,III) oxide
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- published: 22 Oct 2015
- views: 143
63:12
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ: How well do or...
published: 05 Mar 2015
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
DSSS: Determining chemical and microbial Fe(II) oxidation kinetics in situ...
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- published: 05 Mar 2015
- views: 57
1:46
REDOX : iron(II) sulfate oxidation with permanganate ion
Ferrous ion is oxidized to ferric ion by potassium permanganate according to the following...
published: 17 Oct 2011
REDOX : iron(II) sulfate oxidation with permanganate ion
REDOX : iron(II) sulfate oxidation with permanganate ion
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- published: 17 Oct 2011
- views: 11169
0:44
Iron oxide Meaning
Video shows what iron oxide means. The compound obtained by the reaction of oxygen on iron...
published: 23 Apr 2015
Iron oxide Meaning
Iron oxide Meaning
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- published: 23 Apr 2015
- views: 236
9:41
Iron(III) oxide
This page is about a red-colored oxide of iron. For other uses, see red iron.
Iron(III) ox...
published: 31 Aug 2014
Iron(III) oxide
Iron(III) oxide
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- published: 31 Aug 2014
- views: 676
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2:32
Iron(II) oxide
Iron(II) oxide
Iron(II) oxide is the inorganic compound with the formula FeO.Its minera...
published: 22 Jan 2016
Iron(II) oxide
Iron(II) oxide
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- published: 22 Jan 2016
- views: 13
0:33
Ferrous oxide Meaning
Video shows what ferrous oxide means. The chemical compound FeO, iron oxide where iron has...
published: 30 Apr 2015
Ferrous oxide Meaning
Ferrous oxide Meaning
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- published: 30 Apr 2015
- views: 58
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21:04
Copper(II) oxide nanoparticles penetrate into HepG2 cells, exert cytotoxicity via oxidative stress
Jean‐Pascal Piret, University of Namur
published: 07 Apr 2013
Copper(II) oxide nanoparticles penetrate into HepG2 cells, exert cytotoxicity via oxidative stress
Copper(II) oxide nanoparticles penetrate into HepG2 cells, exert cytotoxicity via oxidative stress
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- published: 07 Apr 2013
- views: 203
43:37
Iron
Iron is a chemical element with the symbol Fe (from Latin: ferrum) and atomic number 26. I...
published: 20 May 2014
Iron
Iron
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- published: 20 May 2014
- views: 260656
41:43
The maufacturing of Aluminum
Aluminum isn't found in nature as a pure element. It exhibits relatively high chemical rea...
published: 24 Mar 2016
The maufacturing of Aluminum
The maufacturing of Aluminum
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- published: 24 Mar 2016
- views: 154
28:41
Inorganic Chemical Tests: Gases, Cations and Anions.
Flame Tests: Lithium – Crimson; Sodium – Yellow or Orange; Potassium - Lilac; Calcium - Br...
published: 24 Apr 2016
Inorganic Chemical Tests: Gases, Cations and Anions.
Inorganic Chemical Tests: Gases, Cations and Anions.
- Report rights infringement
- published: 24 Apr 2016
- views: 1048
27:22
C1.3 Lesson2 Iron Extraction with Carbon
C1 AQA Extraction of iron, with some details about Blast furnace and reactions in blast fu...
published: 16 Feb 2015
C1.3 Lesson2 Iron Extraction with Carbon
C1.3 Lesson2 Iron Extraction with Carbon
- Report rights infringement
- published: 16 Feb 2015
- views: 410
31:49
Balancing Chemical Equations Tutorial - Examples & Practice Problems For Test / Exam Review
This video provides a tutorial on how to balance chemical equations such as combustion rea...
published: 14 Feb 2016
Balancing Chemical Equations Tutorial - Examples & Practice Problems For Test / Exam Review
Balancing Chemical Equations Tutorial - Examples & Practice Problems For Test / Exam Review
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- published: 14 Feb 2016
- views: 1207
20:41
Reversible Reactions
Reversible Reactions: In this lesson we will study reversible reactions.
In the above che...
published: 29 Oct 2015
Reversible Reactions
Reversible Reactions
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- published: 29 Oct 2015
- views: 228
57:07
Mod-03 Lec-19 Metal and Metal Oxide Nanowires - II
Nano structured materials-synthesis, properties, self assembly and applications by Prof. A...
published: 02 Sep 2014
Mod-03 Lec-19 Metal and Metal Oxide Nanowires - II
Mod-03 Lec-19 Metal and Metal Oxide Nanowires - II
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- published: 02 Sep 2014
- views: 563
115:39
Super Metroid Oxide (Stream)
So yeah. . . I decided to stream Oxide for fun. This hack still holds up to the goofiness ...
published: 11 Aug 2014
Super Metroid Oxide (Stream)
Super Metroid Oxide (Stream)
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- published: 11 Aug 2014
- views: 1706
Copper(II) oxide nanoparticles penetrate into HepG...
Iron...
The maufacturing of Aluminum...
Inorganic Chemical Tests: Gases, Cations and Anion...
C1.3 Lesson2 Iron Extraction with Carbon...
Balancing Chemical Equations Tutorial - Examples &...
Reversible Reactions...
Mod-03 Lec-19 Metal and Metal Oxide Nanowires - II...
Super Metroid Oxide (Stream)...
photo: Public Domain / NASA
[Survey]: Poll Reveals A Majority Believe 1969 Moon Landing Was Faked
Edit WorldNews.com 21 Jul 2016
A published survey found a majority of those questioned believe the Apollo 11 Moon landing was in fact faked, according to a Mirror report Thursday.The poll discovered the 25 to 34 age group as those most likely to believe the moon landing never happened, with 73 percent of those falling in that group considering the entire thing to be a highly elaborate hoax ... – WN.com, Jack Durschlag. ....
photo: via YouTube
![[Video]: Syrian rebels ‘mistakenly’ beheaded Palestinian boy](http://web.archive.org./web/20160721230758im_/http://cdn4.wn.com/ph/img/12/59/267ab78c5fda7d58737daa1fb634-medium.jpg "[Video]: Syrian rebels ‘mistakenly’ beheaded Palestinian boy")
Syrian rebels ‘mistakenly’ beheaded Palestinian boy
Edit WorldNews.com 21 Jul 2016
Humanity has reached an all-time low as the video of Syrian rebels ‘mistakenly’ beheading a 12-year-old boy identified as ‘Abdullah Issa’ has surfaced on the internet. . The shocking video, which is currently viral on social media, shows a harassed and frightened boy taunted and later beheaded in a truck by five grown men ... The rebels are identified to be a troop from the Nour al-Din al-Zinki Movement ... WN.com, Kalyani. ....
photo: AP / Joshua Paul
MH370 search team: We’ve been looking in the wrong place
Edit Indian Express 21 Jul 2016photo: ABr / Charles Rex Arbogast
Officer shoots caretaker of autistic man playing outside
Edit The Miami Herald 21 Jul 2016
When a 23-year-old autistic man carrying a toy truck wandered from a mental health center out into the street Monday, a worker there named Charles Kinsey went to retrieve him. A few minutes later the autistic man was still sitting cross-legged blocking the roadway while playing with the small, rectangular white toy ... “He’s on his back with his hands in the air trying to convince the other guy to lie down ... “It was so surprising ... ....
photo: AP / Carolyn Kaster, File
[VIDEO]:Billionaire Mark Cuban Has Some Fun At Donald Trump's Expense On Colbert
Edit WorldNews.com 21 Jul 2016
Cuban has harshly slammed the GOP’s nominee in the past, claiming he’s not as wealthy as he claims and he’s not all that good a businessman, the report said ... “Not just the air.””Your companies fail so often, you must’ve gone to business school at Trump University,” Cuban burned.“Oh, Donald ― he just dropped you like one of your first two wives,” Colbert chimed in ... ....
« back to news headlines
Roger Ailes is out as head of Fox News, Fox Business
Edit The Indiana Times 22 Jul 2016
NEW YORK (AP) — Roger Ailes is out as chief executive at Fox News Channel, his career at the network he built from scratch and ran with an iron hand for nearly 20 years over with stunning swiftness following allegations ... ....
Ailes is out as Fox News head, Murdoch named acting chief
Edit The Indiana Times 22 Jul 2016
NEW YORK — Roger Ailes is out as chief executive at Fox News Channel, his career at the network he built from scratch and ran with an iron hand for nearly 20 years over with stunning swiftness following allegations that ... ....
Roger Ailes out as head of Fox News, Fox Business
Edit Orange County Register 22 Jul 2016
Roger Ailes is out as chief executive at Fox News Channel and Fox Business, his career at the networks he built from scratch and ran with an iron hand for nearly 20 years over with stunning swiftness following allegations that he forced out a former... ....
The Geeky Hooker of Comic-Con will make you feel good
Edit Press Telegram 22 Jul 2016
SAN DIEGO >> Something caught Aimee Hartel's eye as she and her 14-year-old son Ayden walked past a decorative planter outside the Omni Hotel near the San Diego Convention Center Thursday on the first day of this year's San Diego Comic-Con International. "It's Iron Man," he announced, pulling out a tiny red crocheted creation fashioned after the Avenger ... ....
Rangers have left Celtic playing catch-up says Ibrox stalwart
Edit Scotsman 22 Jul 2016
Brendan Rodgers has allowed Rangers to steal a march on the defending champions, according to former Ibrox player and coach Ian Durrant ... “I've been surprised by it. But if you know Brendan Rodgers, the English league is a wee bit later than us in terms of declaring their squads and maybe he has a couple of irons in the fire. I think he'll need to act quick because you want to get the team bedded in ... He's added competition ... ....
Alacer Gold Announces Further Exploration Results for the Copler District
Edit Stockhouse 21 Jul 2016
Rod Antal, Alacer’s President & Chief Executive Officer, stated, “We’ve taken a disciplined approach to our exploration program and have focused on the discovery of satellite leachable oxide mineralization that has the potential to provide supplemental feed to the existing Çöpler heap leach pad ... 11.0m @ 1.00g/t Au from 138.0m (oxide). (oxide) ... (oxide) ... (oxide). (oxide). 28.0m @ 4.00g/t Au from 113.0m (oxide) ... (oxide) ... (oxide)....
P450 redox partner interactions [Biophysics and Computational Biology]>
Edit PNAS 21 Jul 2016
The heme iron of cytochromes P450 must be reduced to bind and activate molecular oxygen for substrate oxidation. Reducing equivalents are derived from a redox partner, which requires the formation of a protein–protein complex. A subject of increasing discussion is the role that redox partner binding plays, if any, in... ....
2016 07 21 Exploration Update - Cakmaktepe North - FINAL (Alacer Gold Corp)
Edit Public Technologies 21 Jul 2016
Rod Antal, Alacer's President & Chief Executive Officer, stated, "We've taken a disciplined approach to our exploration program and have focused on the discovery of satellite leachable oxide mineralization that has the potential to provide supplemental feed to the existing Çöpler heap leach pad ... (oxide) (oxide) ... (sulfide) (oxide) (sulfide) (oxide) (oxide) (oxide) ... (oxide) (oxide) ... (oxide) (oxide) (oxide) (oxide) (oxide) ... (oxide)....
Alacer Gold Announces Further Exploration Results for The Çöpler District (Alacer Gold Corp)
Edit Public Technologies 21 Jul 2016
Rod Antal, Alacer's President & Chief Executive Officer, stated, "We've taken a disciplined approach to our exploration program and have focused on the discovery of satellite leachable oxide mineralization that has the potential to provide supplemental feed to the existing Çöpler heap leach pad ... (oxide) (oxide) ... (sulfide) (oxide) (sulfide) (oxide) (oxide) (oxide) ... (oxide) (oxide) ... (oxide) (oxide) (oxide) (oxide) (oxide) ... (oxide)....
Integration of Novel Materials with Silicon Chips Makes New ‘Smart’ Devices Possible (North Carolina State University)
Edit Public Technologies 21 Jul 2016
The novel functional materials are oxides, including several types of materials that, until now, could not be integrated onto silicon chips ... 'These novel oxides are normally grown on materials that are not compatible with computing devices,' says Jay Narayan, the John C ... a titanium nitride platform, for use with nitride-based electronics; and yttria-stabilized zirconia, for use with oxide-based electronics....
07/21/2016 2Q16 Production Report (Vale SA)
Edit Public Technologies 21 Jul 2016
(Vale) reached 86.8 Mt of iron ore production1 in the second quarter of 2016 (2Q16), 9.3 Mt higher than in 1Q16, mainly due to the good performance of the Northern System ... 1 Excluding Samarco's attributable production and including iron ore acquired from third parties ... Commissioning of the Moatize II plant is almost concluded and its start-up is expected by early August ... Iron ore1....
Deposition of organic nitrogen [Letters (Online Only)]>
Edit PNAS 21 Jul 2016
In PNAS, we (1) highlight changes in the balance of oxidized and reduced nitrogen contributions to United States reactive nitrogen deposition, pointing out that decreases in nitrogen oxides (NOx) emissions, combined with modest growth in ammonia emissions, have altered the inorganic nitrogen deposition budget from majority deposition by oxidized species... ....
2Q16 Production Report (Vale SA)
Edit Public Technologies 21 Jul 2016
Vale reached 86.8 Mt of iron ore production in the second quarter of 2016 (2Q16), 9.3 Mt higher than in 1Q16, mainly due to the good performance of the Northern System. ... In June, the total mine movement in Mozambique reached a new monthly record of 12.7 Mt due to higher equipment productivity and the development of new mining areas which will feed the Moatize II coal handling and preparation plant....
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