According to Le Chatelier's principle, a change in temperature, pressure, or concentration of a system at equilibrium will shift the equilibrium to counteract the change.

1. Effect of Temperature: The given reaction is exothermic ($\Delta_r H = -X \text{ kJ}$ is negative). For exothermic reactions, decreasing the temperature favours the forward reaction as the system shifts to produce more heat.
2. Effect of Pressure: The forward reaction proceeds with a decrease in the number of gaseous moles (2 moles of reactants form 1 mole of product). An increase in pressure favours the direction that produces fewer moles of gas to reduce the pressure. Therefore, high pressure favours the forward reaction. Thus, low temperature and high pressure will favour maximum product formation.