A sample of gas in which [h2s] = 5.76 m is heated to 1400 k in a sealed vessel. after chemical equilibrium has been achieved, what is the value of [h2s]? assume no h2 or s2 was present in the original sample.

According to the equation reaction:

2H2S (g) ↔ 2H2 (g) + S2 (g)

initial m 5.76m 0 0

change - X + X + X

final (5.76-X) X X

and when we have Kc = 2.2x10^-4 (given) so, by substitution:

Kc = [H2]^2*[S2]/[H2S]^2

2.2x10^-4 = (X^2*X) / (5.76-X)

∴X = 0.11 m

∴[H2S] = 5.76 - X = 5.76 - 0.11 = 5.65 m