Question:

If the activation energy for the forward reaction is \( 150 \, \text{kJ/mol} \) and that of the reverse reaction is \( 260 \, \text{kJ/mol} \), what is the enthalpy change for the reaction?

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In exothermic reactions, the activation energy of the reverse reaction is higher than that of the forward reaction, resulting in a negative enthalpy change (\( \Delta H \)).
Updated On: Apr 14, 2025
  • \( 410 \, \text{kJ/mol} \)
  • \( -110 \, \text{kJ/mol} \)
  • \( 110 \, \text{kJ/mol} \)
  • \( -410 \, \text{kJ/mol} \)
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The Correct Option is B

Solution and Explanation

The enthalpy change (ΔH) for a reaction is the difference between the activation energy of the forward reaction (Ea_forward) and the activation energy of the reverse reaction (Ea_reverse):

ΔH = Ea_forward - Ea_reverse

Given:

  • Ea_forward = 150 kJ/mol
  • Ea_reverse = 260 kJ/mol

Substituting the values:

ΔH = 150 kJ/mol - 260 kJ/mol

ΔH = -110 kJ/mol

Therefore, the enthalpy change for the reaction is -110 kJ/mol.

Final Answer: -110 kJ/mol

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