\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftarrows 2 \mathrm{NO}_{2}(g) \quad \Delta \mathrm{H}^{\circ}=+58 \mathrm{~kJ} / \mathrm{mol}_{\mathrm{rxn}} . The chemical equation shown above represents the reversible reaction in which N,0¿(g) isconverted into NO,(g). The value of

the equilibrium constant, K, for this reaction is equal to0.005 at 25°C. If the temperature of the reaction vessel is increased from 25°C to 100°C, do you predict that the value of K will decrease, increase, or remain the same? Justify your answer.