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)#

1 Answer
Oct 1, 2017

Answer:

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?