N2O4(g) ↔ 2NO2(g) ΔH = +ve In the reaction above, an increase in temperature will

The given chemical equation shows a reversible reaction where nitrogen dioxide (NO2) and dinitrogen oxide (N2O4) are in equilibrium. The reaction is endothermic, which means it absorbs heat. According to Le Chatelier's principle, an increase in temperature will favor the endothermic reaction, which absorbs heat. As a result, the equilibrium will shift in the direction that consumes heat, which in this case is the forward reaction. Therefore, an increase in temperature will shift the equilibrium to the right, favoring the formation of more NO2 gas and reducing the concentration of N2O4. As a result, the equilibrium constant (K) for this reaction, which is the ratio of products to reactants at equilibrium, will increase. Thus, the correct answer is "increase the value of the equilibrium constant."