## Introductory Chemistry (5th Edition)

The equilibrium constant value for that reaction is equal to $0.0987$.
1. Write the equilibrium constant expression: $K_{eq} = \frac{[Products]}{[Reactants]} = [NH_3][H_2S]$ ** Notice: we do not consider the $NH_4HS$ concentration, because it is a solid. 2. Using the given values, calculate the $K_{eq}$: $K_{eq} = 0.278 \times 0.355 = 0.0987$