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When iron react with concentrated nitric acid passivity occurs whats the passivity?
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+ Chemical reactions
+ Iron
+ Acids
+ Chemistry
+ Organic chemistry
+ Hydrochloric acid
+ Nitric acid
Posted by
May Chen
When iron react with concentrated nitric acid passivity occurs whats the passivity?
Conc nitric acid being a strong oxidising agent, converts the metal into ferric oxide which forms an insoluble protective coating on it.Since the metal loses contact with acid, the reaction stops.A chemically active metal becomes passive- un reactive.
Conc nitric acid being a strong oxidising agent, converts the metal into ferric oxide which forms an insoluble protective coating on it.Since the metal loses contact with acid, the reaction stops.A chemically active metal becomes passive- un reactive.
Treating many metals such as iron with a strong oxidising agent such as conc. nitric acid, produces a passive state in the metal, such that no further interaction with the nitric acid occurs. This induced passive state is caused by the oxidation of ferric nitrate to the oxide which resists further acid attack. Thus:
Fe + 3HNO3 = Fe(NO3)3 + 3H
However, the highly reactive nascent H extracts the oxygen from the ferric nitrate to form a film of insoluble and non-reactive ferric oxide at the surface that is responsible for the passive state of elemental iron.
2Fe(NO3)3 + 18H = Fe2O3 + 6NO + 9H2O
Combining these reactions into a single chemical equation to reflect what occurs at the surface of the iron metal, we get:
Fe+3HNO3+15H+Fe(NO3)3=Fe2O3+6NO+9H2O
Thus, the passivation of iron requires both the presence of conc. nitric acid and the generation of nascent hydrogen. Use of dilute acid produces the normal reaction of a metal with an acid to produce the water soluble ferric nitrate plus hydrogen gas.
Treating many metals such as iron with a strong oxidising agent such as conc. nitric acid, produces a passive state in the metal, such that no further interaction with the nitric acid occurs. This induced passive state is caused by the oxidation of ferric nitrate to the oxide which resists further acid attack. Thus:
Fe + 3HNO3 = Fe(NO3)3 + 3H
However, the highly reactive nascent H extracts the oxygen from the ferric nitrate to form a film of insoluble and non-reactive ferric oxide at the surface that is responsible for the passive state of elemental iron.
2Fe(NO3)3 + 18H = Fe2O3 + 6NO + 9H2O
Combining these reactions into a single chemical equation to reflect what occurs at the surface of the iron metal, we get:
Fe+3HNO3+15H+Fe(NO3)3=Fe2O3+6NO+9H2O
Thus, the passivation of iron requires both the presence of conc. nitric acid and the generation of nascent hydrogen. Use of dilute acid produces the normal reaction of a metal with an acid to produce the water soluble ferric nitrate plus hydrogen gas.
Conc nitric acid being a strong oxidising agent, converts the metal into ferric oxide which forms an insoluble protective coating on it.Since the metal loses contact with acid, the reaction stops.A chemically active metal becomes passive- un reactive.
Conc nitric acid being a strong oxidising agent, converts the metal into ferric oxide which forms an insoluble protective coating on it.Since the metal loses contact with acid, the reaction stops.A chemically active metal becomes passive- un reactive.
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Treating many metals such as iron with a strong oxidising agent such as conc. nitric acid, produces a passive state in the metal, such that no further interaction with the nitric acid occurs. This induced passive state is caused by the oxidation of ferric nitrate to the oxide which resists further acid attack. Thus:
Fe + 3HNO3 = Fe(NO3)3 + 3H
However, the highly reactive nascent H extracts the oxygen from the ferric nitrate to form a film of insoluble and non-reactive ferric oxide at the surface that is responsible for the passive state of elemental iron.
2Fe(NO3)3 + 18H = Fe2O3 + 6NO + 9H2O
Combining these reactions into a single chemical equation to reflect what occurs at the surface of the iron metal, we get:
Fe+3HNO3+15H+Fe(NO3)3=Fe2O3+6NO+9H2O
Thus, the passivation of iron requires both the presence of conc. nitric acid and the generation of nascent hydrogen. Use of dilute acid produces the normal reaction of a metal with an acid to produce the water soluble ferric nitrate plus hydrogen gas.
Treating many metals such as iron with a strong oxidising agent such as conc. nitric acid, produces a passive state in the metal, such that no further interaction with the nitric acid occurs. This induced passive state is caused by the oxidation of ferric nitrate to the oxide which resists further acid attack. Thus:
Fe + 3HNO3 = Fe(NO3)3 + 3H
However, the highly reactive nascent H extracts the oxygen from the ferric nitrate to form a film of insoluble and non-reactive ferric oxide at the surface that is responsible for the passive state of elemental iron.
2Fe(NO3)3 + 18H = Fe2O3 + 6NO + 9H2O
Combining these reactions into a single chemical equation to reflect what occurs at the surface of the iron metal, we get:
Fe+3HNO3+15H+Fe(NO3)3=Fe2O3+6NO+9H2O
Thus, the passivation of iron requires both the presence of conc. nitric acid and the generation of nascent hydrogen. Use of dilute acid produces the normal reaction of a metal with an acid to produce the water soluble ferric nitrate plus hydrogen gas.
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