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Standard XII

Chemistry

Collision Theory

If a reaction...

Question

If a reaction, $A + B \to C$ is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy 70 kJ/mol, the activation energy for the reverse reaction is (in kJ/mol):

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Solution

$Δ H = - 30$ kJ/mol, means that the reactants are at an energy of $30$ kJ/mol, higher than the products.
The activation energy of the forward reaction is equal to the difference in energy between the reactants and the activated complex.
Hence, the activation energy of the backward reaction would be the sum of the energy difference between the reactants and the products and the activation energy of the forward reaction i.e.,
$30 + 70 = 100$ kJ/mol

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If a reaction, A+B→C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy 70 kJ/mol, the activation energy for the reverse reaction is (in kJ/mol):

If a reaction, $A + B \to C$ is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy 70 kJ/mol, the activation energy for the reverse reaction is (in kJ/mol):