Question

What molar quantity of carbon monoxide is required to reduce a `160*g` mass of `Fe_2O_3`?

We follow the stoichiometric equation...

`Fe_2O_3(s) + 3CO(g) stackrel(Delta)rarr2Fe(s) + 3CO_2(g)`

Answer 1

Look at the stoichiometry of your equation....

Explanation:

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

And this explicitly tells me that heating `160*g` `"ferric oxide"` in the presence of `84*g` `"carbon monoxide gas"` results in the formation of `112*g` of (molten) iron and `152*g` of `"carbon dioxide gas"`. As is always observed in any chemical reaction, MASS is conserved. Is it conserved here?

So you gots `2.4*mol` of iron....`3xx2.4*mol` of carbon monoxide were necessary, and clearly `1.2*mol` of `"ferric oxide"` were required. You will have to fill in the appropriate masses. Can you do so?