Answer
The reaction will proceed in the reverse direction, producing more reactants. (to the left)
Work Step by Step
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.
