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

1. Effect of Temperature: Since the reaction is exothermic ($\Delta H$ is negative), low temperature will shift the equilibrium towards the product side.2. Effect of Pressure: The reactant has 2 moles of gas ($1+1$) and the product has 1 mole. Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, i.e., the product side.Optimal conditions: Low temperature and high pressure.