Answer
Since the calculated $Q_p$ for the initial conditions is less than the $K_p$ for this equilibrium at this temperature, the pressure of the products: $PCl_3$ and $Cl_2$ will increase, and the pressure of the reactant: $PCl_5$ will decrease.
Work Step by Step
1. Write the equilibrium constant expression:
- The exponent of each concentration is equal to its balance coefficient.
$$K_P = \frac{[Products]}{[Reactants]} = \frac{P_{ PCl_3 }P_{ Cl_2 }}{P_{ PCl_5 }}$$
2. Calculate the initial $Q_p$:
$$Q_P = \frac{(0.223)(0.111)}{0.177} = 0.14$$
3. Since $Q_{p \space initial} < K_p$, product will be formed, consuming products.
The pressures of the products will increase, and the same of the reactants will decrease.
