What is the limiting reagent and the moles of #CO_2# formed when 11 moles #CS_2# reacts with 18 moles #O_2# to produce #CO_2# gas and #SO_2# gas at STP?
The equation is #CS_2(g) + 3O_2(g) -> CO_2(g) + 2SO_2(g)# ?
The equation is
1 Answer
Explanation:
Limiting reagent problems are all about using the mole ratio that exists between the reactants to determine if you have enough of each reactant to allow for their complete consumption.
Take a look at the balanced chemical equation for your reaction
#"CS"_text(2(l]) + color(red)(3)"O"_text(2(g]) -> "CO"_text(2(g]) + 2"SO"_text(2(g])#
The
You can thus distinguish between three possible cases here
-
if you have less than
#color(red)(3)# moles of oxygen gas for every mole of carbon disulfide, oxygen gas will be the limiting reagent -
if you have more than
#color(red)(3)# moles of oxygen gas for every mole of carbon disulfide, carbon disulfide gas will be the limiting reagent -
if you have exactly
#color(red)(3)# moles of oxygen gas for every mole of carbon disulfide, you are not dealing with a limiting reagent*
The problem tells you that
#11 color(red)(cancel(color(black)("moles CS"_2))) * (color(red)(3)" moles O"_2)/(1color(red)(cancel(color(black)("mole CS"_2)))) = "33 moles O"_2#
in order to be completely consumed. Since you don't have enough oxygen gas present, you can say that oxygen gas will be the limiting reagent.
Now, how much carbon disulfide will actually react? Once again, use the mole ratio that exists between the two reactants
#18 color(red)(cancel(color(black)("moles O"_2))) * "1 mole CS"_2/(color(red)(3)color(red)(cancel(color(black)("moles O"_2)))) = "6 moles CS"_2#
So,
#6color(red)(cancel(color(black)("moles CS"_2))) * "1 mole CO"_2/(1color(red)(cancel(color(black)("mole CS"_2)))) = color(green)("6 moles CO"_2)#