Question

For an endothermic reaction where ΔH represents the enthalpy of the reaction in kj/mol. the minimum value for the energy of activation will be

Answer 1

For endothermic reaction the forward activation energy is greater than the backward activation energy and for the reaction the value of delta H is positive hence the minimum amount of activation energy should be greater than the delta H of the reaction

Answer 2

Answer:

Activation energy: E

a

is the energy that must be possessed by the molecules in excess to the average energy at a given temperature to enter a chemical reaction.

Relation between activation energy and enthalpy of a reversible reaction:

If the reaction is endothermic in forward direction, then E

a(backward)

=E

a(forward)

+ΔH

If the reaction is exothermic in forward direction then E

a(backward)

=E

a(forward)

+ΔH

For an endothermic reaction, where ΔH represents the enthalpy of

the reaction in kJmol

−1

, the minimum value for the energy of activation will be slightly more than ΔH.

Explanation:

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