$delta_H$ at temperature T2 = $delta_H$ at T1 + $delta_{Cp}$(T2 - T1). $delta_{Cp}$ = sum(Cp products) - sum(Cp reactants). This allows calculation of enthalpy at non-standard temperatures. Similarly: $delta_U$(T2) = $delta_U$(T1) + $delta_{Cv}$(T2 - T1). If $delta_{Cp}$ > 0, the reaction becomes more endothermic (or less exothermic) with increasing temperature. If $delta_{Cp}$ < 0, it becomes more exothermic with increasing temperature. JEE rarely tests this directly but it appears in advanced problems.