A sample of pure solid calcium carbonate, \(\text{CaCO}_3(s)\), is placed in an evacuated, rigid container and heated to \(1000\text{ K}\), where it undergoes thermal decomposition according to the following reversible process:

\[\text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g)\]

At this temperature, the equilibrium constant is \(K_p = 0.050\). Additional \(\text{CO}_2(g)\) is added to the container such that the instantaneous partial pressure of carbon dioxide is \(P_{\text{CO}_2} = 0.20\text{ atm}\) in the presence of both solids. Which of the following gives the correct expression for the reaction quotient, \(Q_p\), and correctly predicts the direction of the net process required to establish equilibrium?