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

1 Answer
Feb 20, 2016

Answer:

#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.