## Chemistry: Molecular Approach (4th Edition)

1. Calculate the $Q_p$ for that reaction: - The exponent of each concentration is equal to its balance coefficient. $$Q_p = \frac{[Products]}{[Reactants]} = \frac{P_{ H_2 } ^{ 2 }P_{ S_2 }}{P_{ H_2S } ^{ 2 }}$$ 2. Substitute the values and calculate the constant value: $$Q_p = \frac{( 0.055 )^{ 2 }( 0.445 )}{( 0.112 )^{ 2 }} = 0.11$$ $Q_p \gt K_p$, therefore, the reaction mixture is not at equilibrium, and the reverse reaction is going to be favored, producing more reactants.