Consider the reaction:
$$COCl_2(g) \rightleftharpoons CO(g) + Cl_2(g)$$
$$K_p = 1.5 \times 10^{-12} \text{ at } 25^\circ C$$
At equilibrium, this reaction is
At equilibrium, the rates of $\rightarrow$ and $\leftarrow$ reaction are equal.
At equilibrium, reactant and product concentrations are equal.
Once the reaction has reached equilibrium, all reaction stops.
Increasing the temperature changes the $K_p$ value for this reaction.
Adding $COCl_2(g)$ changes the value of $K_p$ for this reaction.
For the reaction: $CO(g) + Cl_2(g) \rightleftharpoons COCl_2(g)$, the value of $K_p$ is equal to
