Which one of the following conditions will favour maximum formation of the product in the reaction, $A_2(g) + B_2(g) \rightleftharpoons 2X_2(g) \Delta H = -X \text{ kJ}$?

For the reaction $A_2(g) + B_2(g) \rightleftharpoons 2X_2(g); \Delta H = -x \text{ kJ}$, increasing pressure shifts equilibrium towards the side with fewer moles of gas (forward direction). Decreasing temperature shifts equilibrium in the exothermic direction (forward direction). Thus, high pressure and low temperature favour maximum formation of the product.