“Reacting iron powder with dilute nitric acid will produce Iron III Nitrate, nitrous oxide & water (the nitric acid oxidising the iron to the Fe3+ cation). The reaction proceeds slowly.
Fe + 4 HNO3 → Fe(NO3)3) + NO + 2H2O
Concentrated nitric acid renders the iron passive though - a small amount of Fe2O3 is formed and coats the metal, but that cannot be oxidised any further and the reaction then stops.” -Gary McAdam
“Reacting iron powder with dilute nitric acid will produce Iron III Nitrate, nitrous oxide & water (the nitric acid oxidising the iron to the Fe3+ cation). The reaction proceeds slowly.
Fe + 4 HNO3 → Fe(NO3)3) + NO + 2H2O
Concentrated nitric acid renders the iron passive though - a small amount of Fe2O3 is formed and coats the metal, but that cannot be oxidised any further and the reaction then stops.” -Gary McAdam
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.
If you compare iron to zinc, I think the products produced would similarly depend on the concentration of nitric acid. These could range from NO, NO2, iron(III)nitrate and ammonium nitrate and an oxide coating (Fe2O3) of iron ( in the case of concentrated acid, creating passivity as a direct result of the oxidizing ability of nitric acid). Also H2O would be formed.
If you compare iron to zinc, I think the products produced would similarly depend on the concentration of nitric acid. These could range from NO, NO2, iron(III)nitrate and ammonium nitrate and an oxide coating (Fe2O3) of iron ( in the case of concentrated acid, creating passivity as a direct result of the oxidizing ability of nitric acid). Also H2O would be formed.
The resulting compounds would be ferric nitrate, nitric oxide, and water.
The resulting compounds would be ferric nitrate, nitric oxide, and water.
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If we react iron with dilute nitric acid then,
3Fe + 8HNO3 →3Fe(NO3)2 + 4H2O + 2NO
If we react iron with concentrated nitric acid then,
Fe + 6HNO3 →Fe(NO3)3 + 3H2O + 3NO2
If we react iron with dilute nitric acid then,
3Fe + 8HNO3 →3Fe(NO3)2 + 4H2O + 2NO
If we react iron with concentrated nitric acid then,
Fe + 6HNO3 →Fe(NO3)3 + 3H2O + 3NO2
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I am very sorry to say this that many students gave a wrong answer to this question.originally,Fe + conc.HNO3 remains passive.
Fe + dil.HNO3 gives iron nitrate along with NO.
I am very sorry to say this that many students gave a wrong answer to this question.originally,Fe + conc.HNO3 remains passive.
Fe + dil.HNO3 gives iron nitrate along with NO.
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Iron is rendered passive by concentrated nitric acid.
I believe that dilute nitric will dissolve it, but you may get ferrous nitrate and some ammonium nitrate.
Iron is rendered passive by concentrated nitric acid.
I believe that dilute nitric will dissolve it, but you may get ferrous nitrate and some ammonium nitrate.
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Hey! Check this What would the reaction of iron and nitric acid?
“Reacting iron powder with dilute nitric acid will produce Iron III Nitrate, nitrous oxide & water (the nitric acid oxidising the iron to the Fe3+ cation). The reaction proceeds slowly.
Fe + 4 HNO3 → Fe(NO3)3) + NO + 2H2O
Concentrated nitric acid renders the iron passive though - a small amount of Fe2O3 is formed and coats the metal, but that cannot be oxidised any further and the reaction then stops.” -Gary McAdam
Hey! Check this What would the reaction of iron and nitric acid?
“Reacting iron powder with dilute nitric acid will produce Iron III Nitrate, nitrous oxide & water (the nitric acid oxidising the iron to the Fe3+ cation). The reaction proceeds slowly.
Fe + 4 HNO3 → Fe(NO3)3) + NO + 2H2O
Concentrated nitric acid renders the iron passive though - a small amount of Fe2O3 is formed and coats the metal, but that cannot be oxidised any further and the reaction then stops.” -Gary McAdam
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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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According to the Russian Wikipedia, the reaction goes as follows:
Fe3O4+10HNO3⟶3Fe(NO3)3+NO2+5H2O
Since Fe3O4 is often written out as Fe2O3⋅FeO, why don't we have instead
Fe3O4+ 8 HNO3⟶Fe(NO3)2+2Fe(NO3)3+4H2O
According to the Russian Wikipedia, the reaction goes as follows:
Fe3O4+10HNO3⟶3Fe(NO3)3+NO2+5H2O
Since Fe3O4 is often written out as Fe2O3⋅FeO, why don't we have instead
Fe3O4+ 8 HNO3⟶Fe(NO3)2+2Fe(NO3)3+4H2O
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If you compare iron to zinc, I think the products produced would similarly depend on the concentration of nitric acid. These could range from NO, NO2, iron(III)nitrate and ammonium nitrate and an oxide coating (Fe2O3) of iron ( in the case of concentrated acid, creating passivity as a direct result of the oxidizing ability of nitric acid). Also H2O would be formed.
If you compare iron to zinc, I think the products produced would similarly depend on the concentration of nitric acid. These could range from NO, NO2, iron(III)nitrate and ammonium nitrate and an oxide coating (Fe2O3) of iron ( in the case of concentrated acid, creating passivity as a direct result of the oxidizing ability of nitric acid). Also H2O would be formed.
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Gives out a yellow showery Sparks and produces a black solid
Gives out a yellow showery Sparks and produces a black solid
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