Chemistry: Molecular Approach (4th Edition)

The reverse reaction is favored, producing more solid $NH_4HS$.
1. Calculate the $Q_p$ for that reaction: - The exponent of each concentration is equal to its balance coefficient. $$Q_C = \frac{[Products]}{[Reactants]} = {[ NH_3 ][ H_2S ]}$$ 2. Substitute the values and calculate $Q_c$: $$Q_C = {( 0.166 )( 0.166 )} = 0.0276$$ $Q_c \gt K_c$, therefore, the reverse reaction is favored, producing more solid $NH_4HS$.