The solid NH4HS is in equilibrium with the gases NH3 and H2S. An equilibrium mixture contains solid NH4HS, 9.6×10−2 M NH3, and 0.026M H2S.
NH4HS(s)⇌NH3(g)+H2S(g)

What is the value of the equilibrium constant, Kc, for the reaction?

Question

The solid NH4HS is in equilibrium with the gases NH3 and H2S. An equilibrium mixture contains solid NH4HS, 9.6×10−2 M NH3, and 0.026M H2S.
NH4HS(s)⇌NH3(g)+H2S(g)

What is the value of the equilibrium constant, Kc, for the reaction?

anonymous · Answer

I think I figured it out: 

Kc = 0.096 x 0.026 = $$2.5×10^{-3}$$

anonymous · Answer

Yes that's correct. 
$$K_c=\frac{ Products }{ Reactants }=[NH_3]*[H_2S]=(0.096)(0.026)$$
If it's a solid or liquid it is not included in the formula, so we leave out our reactant in this case.