Use the table to answer the question.
Reaction CH4 + 4Cl2 → CCl4 + 4HCl
Reactants Products
Bonds Present
4 H–C
4 Cl–Cl
4 C–Cl
4 H–Cl
Energy of Bonds Broken (Reactants) / Formed (Products)
4 × 411 kJ/mol
4 × 242 kJ/mol
4 × 327 kJ/mol
4 × 427 kJ/mol
Which statement about the change in bond energy of this reaction is correct?
(1 point)
Responses
The reaction is exothermic because the total bond energy of the reactants is less than the total bond energy of the products.
The reaction is exothermic because the total bond energy of the reactants is less than the total bond energy of the products.
The reaction is exothermic because the energy of each bond in the reactants is greater than the energy of a bond in the products.
The reaction is exothermic because the energy of each bond in the reactants is greater than the energy of a bond in the products.
The reaction is endothermic because the total bond energy of the reactants is greater than the total bond energy of the products.
The reaction is endothermic because the total bond energy of the reactants is greater than the total bond energy of the products.
The reaction is endothermic because the energy of each bond in the reactants is less than the energy of a bond in the products.
The correct statement about the change in bond energy of this reaction is:
The reaction is exothermic because the total bond energy of the reactants is less than the total bond energy of the products.