The standard equilibrium constant $K_p^{\circ }$ for the reaction ${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$ is 16. If the volume of the container is reduced to one half of its original volume, the value of $K_p^{\circ }$ for the reaction at the same temperature will be

Solution:

The value of ${\mathrm{K}}_{\mathrm{P}}$ remains constant as temperature is not changed.

Temperature affects the value of the equilibrium constant, Kp. For exothermic and endothermic processes, the variation is different. When temperature rises, the equilibrium for an endothermic forward reaction shifts towards the right and favours the production of additional products, increasing the value of kp in the process.