Consider a chemical reaction where the total enthalpy of the...

Given that the total enthalpy of the products is greater than the total enthalpy of the reactants, $H_P > H_R$.

The enthalpy change for the reaction is given by $\Delta_r H = H_P - H_R$.

Since $H_P > H_R$, it follows that $\Delta_r H > 0$. Thus, the enthalpy change is positive, making statement (B) correct and statement (D) incorrect.

A positive enthalpy change indicates that the reaction is endothermic, meaning heat is absorbed by the system. Therefore, statement (A) is incorrect.

At constant pressure, the heat exchanged is equal to the enthalpy change, $q_p = \Delta_r H$. Since $\Delta_r H > 0$, we have $q_p > 0$, which means heat is absorbed by the system. Thus, statement (C) is correct.

Therefore, only statements (B) and (C) are correct.

Answer: (B) and (C) only