Why does enthalpy change differ in a chemical reaction because of temperature? If enthalpy is a state function, shouldn't the change in enthalpy be the same between a given initial and final state, regardless of how the change took place? Kirchoff's equation describes this variation as
$$\Delta H_{T_2} = \Delta H_{T_1} + \Delta C_p (T_2 - T_1).$$
I'm guessing that this change in enthalpy change is only because of the variation in $C_p$, but I'm not too sure about it. Am I completely wrong about this?
From Hess' law, the heat of reaction at temperatures $T_1$ and $T_2$ are related by $$\Delta H_{T_1}=C_{p,\mathrm r}(T_2-T_1)+\Delta H_{T_2}+C_{p,\mathrm p}(T_1-T_2),$$where $C_{p,\mathrm r}$ is the heat capacity of a stoichiometric molar mixture of reactants and $C_{p,\mathrm p}$ is the heat capacity of a stoichiometric molar mixture of products.