Question

How many moles of carbon dioxide are recovered after reduction of a `1000*g` mass of `Fe_2O_3` by `CO`?

Answer 1

`Fe_2O_3(s) + 3CO(g) rarr 2Fe(s) + 3CO_2(g)`

Explanation:

Moles of haematite: `(1000*g)/(159.69*g*mol^-1)` `=` `??` `"moles"`

Given the stoichiometry of the equation, it is a fact that each mole of `Fe_2O_3` requires `3` `"mol"` carbon monoxide gas for reduction of the oxide. And of course the oxidation product is carbon dioxide gas, `3` `mol` for every `2` mole of iron that is reduced. So all I have to do is calculate the number of moles of oxide, and multiply this figure by 3, to give the number of moles of carbon dioxide product.