10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the container. The number of moles of ammonia gas left in the container must be which of the following?

Question

N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. 8.8 d. 6.4
b. 2.4 e. 9.2
c. 7.6

Answer 1

initial moles:
NH3 = 10
N2 = 0
H2 = 0

equilibrium:
N2 = 1.2 moles from problem.
Therefore, H2 must be 3 x 1.2 = 3.6
NH3 must be 10-(2*1.2) = ??

Answer 2

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