Consider the following reaction equation: X(g) + Y(g) ⇌ XY(g); ∆H = + 220KJ mol-1 If the temperature of the system is increased, the

Answer Details

The reaction equation given is X_(g) + Y_(g) ⇌ XY_(g); ∆H = +220KJ mol^-1. The ∆H value is positive which indicates that the reaction is endothermic, meaning that heat is absorbed when the reaction takes place. According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants/products, the system will respond in a way that tends to counteract that change. In this case, if the temperature of the system is increased, the equilibrium position will shift in the direction that absorbs heat. Since the reaction is endothermic, the forward reaction will absorb heat, so the system will favor the forward reaction to absorb the excess heat. Therefore, the forward reaction would be favored if the temperature of the system is increased. Hence, the correct option is "forward reaction would be favored."