= 1.3 M
= 1.65 M
= 0.1 M
0 + 2x = 0.100 M
x = 0.100 M/2
x = 0.05 M
[N2] = 1.30 M - x
[N2] = 1.30 M - 0.05 M
[N2] = 1.25 M
[H2] = 1.65 M - 3x
[H2] = 1.65 M - 3(0.05M)
[H2] = 1.65 M - 0.15 M
[H2] = 1.50 M
Consider the formation of ammonia in two experiments.
(a) To a 1.00-L container at 727°C, 1.30 mol of N 2 and 1.65 mol of H2 are added. At equilibrium, 0.100 mol of NH3 is present. Calculate the equilibrium concentrations of N 2 and H2, and find Kc for the reaction:
2NH3(g) ⇌ N2(g) + 3H2(g)
(b) In a different 1.00-L container at the same temperature, equilibrium is established with 8.34 x 10−2 mol of NH3, 1.50 mol of N2, and 1.25 mol of H2 present. Calculate Kc for the reaction:
NH3(g) ⇌ 1/2N2(g) + 3/2H2(g)
What is the relationship between the Kc values in parts (a) and (b)? Why aren’t these values the same?
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