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For an endothermic reaction, where ΔH represents the enthalpy of reaction in KJ/mol. The higher value for the energy of activation will be equal to which of the following? |
Less than ΔH Zero More than ΔH Equal to ΔH |
More than ΔH |
Activation energy: Ea 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 Ea(backward) = Ea(forward) + ΔH
If the reaction is exothermic in forward direction, then Ea(backward) = Ea(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.
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