Question

During an exothermic reaction, ΔH for the reactants was 890 kJ/mol. Which of the following statements is correct about the ΔH for the products?
A. It is less than 890 kJ/mol because the amount of energy required to break bonds is less than the amount of energy released in forming bonds.

B. It is less than 890 kJ/mol because the amount of energy required to break bonds is greater than the amount of energy released in forming bonds.

C. It is greater than 890 kJ/mol because the amount of energy required to break bonds is less than the amount of energy released in forming bonds.

D. It is greater than 890 kJ/mol because the amount of energy required to break bonds is greater than the amount of energy released in forming bonds.

Answer 1

Answer:-A. It is less than 890 kJ/mol because the amount of energy required to break bonds is less than the amount of energy released in forming bonds.

Explanation: Endothermic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and $\Delta H$ for the reaction comes out to be positive.

Exothermic reactions are defined as the reactions in which energy of the product is lesser than the energy of the reactants. The total energy is released in the form of heat and $\Delta H$ for the reaction comes out to be negative.

In the formation of new bonds more energy is released than is required to break the existing bonds, heat is released.

In the formation of bonds less energy is released than is required to break the existing bonds, heat is absorbed.

Answer 2

Answer: The correct answer is Option A.

Explanation:

Endothermic reactions are defined as the chemical reactions in which energy of products is more than the energy of the reactants. In these reactions, energy is absorbed by the system. The total enthalpy of the reaction $(\Delta H)$ comes out to be positive.

Exothermic reactions are defined as the chemical reactions in which energy of reactants is more than the energy of the products. In these reactions, energy is released by the system. The total enthalpy of the reaction $(\Delta H)$ comes out to be negative.

When in the formation of new bonds, more energy is released than the energy is required to break the existing bonds, then the heat is released and the reaction is exothermic in nature.

When in the formation of bonds, less energy is released than the energy is required to break the existing bonds, then the heat is absorbed and the reaction is endothermic in nature.

We are given:

An exothermic reaction in which energy of the reactants is 890 kJ/mol. In this process, the energy is getting released.

Hence, the correct answer is Option A.