The said question:
Consider the following equilibrium at high temperature:
2H2(g) + S2(g) <--> 2 H2S(g)
Analysis of the contents of a 4.0L flask reveals that there are 5.7 moles of hydrogen gas, 2.4 moles of sulfur gas, and 5.3 moles of hydrogen sulfide gas in the flask at equilibrium. Calculate the equilibrium constant Kc.
Something must be flying way over my head because this question looks incredibly easy. I just find the concentrations of each substance by dividing the given number of moles by 4 and then plug those values into the equilibrium equation.
Anyways here's what i'm doing:
[H2] = 5.7/ 4 = 1.425
[S2] = 2.4/4 = .6
[H2S] = 1.325
and the equilibrium equation
Kc = ([H2S])^2 / ([S2])*([H2])^2
= 1.325^2 / (.6)(1.425^2)
no matter what i try i always seem to get back to 1.44 as being the equilibrium constant, but its not right.