Iron rusts when exposed to oxygen. Iron(II) is produced in the reaction. How many moles of oxygen oxide will react with 2.4 mol of iron in the rusting reaction?

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Iron rusts when exposed to oxygen. Iron(II) is produced in the reaction. How many moles of oxygen oxide will react with 2.4 mol of iron in the rusting reaction?

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Answer 1 · 2017-02-27T07:09:18

Iron has a rich redox chemistry..............

Explanation:

$Fe(s) + 1/2O_2 rarr FeO(s)$

This is a very simplified representation of the oxidation of iron metal. But if there are $2.4*mol$ of iron metal, it should react with $1.2*mol$ of dioxygen gas to give $2.4*mol$ of iron oxide, as per the stoichiometric equation.

When rust occurs on a bridge or on a steel structure, it is a surface phenomenon.

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Iron rusts when exposed to oxygen. Iron(II) is produced in the reaction. How many moles of oxygen oxide will react with 2.4 mol of iron in the rusting reaction?

1 Answer

Explanation:

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