Use the table to answer the question.

Let's analyze the reaction and the associated bond energies provided to determine if the reaction is endothermic or exothermic.

The reaction is: \[ \text{CH}_4 + 4\text{Cl}_2 \rightarrow \text{CCl}_4 + 4\text{HCl} \]

Bonds Present:

• Reactants:

  • 4 H-C bonds
  • 4 Cl-Cl bonds

• Products:

  • 4 C-Cl bonds
  • 4 H-Cl bonds

Energy of Bonds:

• Energy of breaking bonds in reactants:

  • For 4 H-C bonds: \( 4 \times 411 , \text{kJ/mol} = 1644 , \text{kJ/mol} \)
  • For 4 Cl-Cl bonds: \( 4 \times 242 , \text{kJ/mol} = 968 , \text{kJ/mol} \)

  Total energy of bonds broken (reactants): \[ 1644 , \text{kJ/mol} + 968 , \text{kJ/mol} = 2612 , \text{kJ/mol} \]

• Energy of forming bonds in products:

  • For 4 C-Cl bonds: \( 4 \times 327 , \text{kJ/mol} = 1308 , \text{kJ/mol} \)
  • For 4 H-Cl bonds: \( 4 \times 427 , \text{kJ/mol} = 1708 , \text{kJ/mol} \)

  Total energy of bonds formed (products): \[ 1308 , \text{kJ/mol} + 1708 , \text{kJ/mol} = 3016 , \text{kJ/mol} \]

Change in Bond Energy:

• Total energy of bonds broken (reactants) = 2612 kJ/mol
• Total energy of bonds formed (products) = 3016 kJ/mol

Calculation of ΔH:

To find whether the reaction is endothermic or exothermic, we use the formula: \[ \Delta H = \text{Energy of bonds broken} - \text{Energy of bonds formed} \] \[ \Delta H = 2612 , \text{kJ/mol} - 3016 , \text{kJ/mol} = -404 , \text{kJ/mol} \]

Since ΔH is negative, the reaction is exothermic.

Conclusion:

The correct answer is: The reaction is exothermic because the total bond energy of the reactants is less than the total bond energy of the products.