Consider a chemical reaction where the total enthalpy of the products is greater than the total enthalpy of the reactants. Which of the following statements are correct for this process? (A) The reaction is exothermic in nature. (B) The enthalpy change ( _r H ) is positive. (C) Heat is absorbed by the system at constant pressure ( q_p > 0 ). (D) The enthalpy change ( _r H ) is negative. Choose the correct answer from

Step-by-step solution

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 _r H = H_P - H_R . Since H_P > H_R , it follows that _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