For an endothermic reaction, energy of activation is $E_{a}$ and enthalpy of reaction is $Δ H$ (both of these in kJ/mol). Minimum value of $E_{a}$ will be:

Less than $Δ H$

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Equal to $Δ H$

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More than $Δ H$

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Equal to zero

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Solution

The correct option is C
More than $Δ H$

In endothermic reactions, energy of reactants is less than that of the products.Potential energy diagram for endothermic reactions is

Where
$E_{a}$ = activation energy of forward reaction
$E_{a}^{'}$ = activation energy of backward reaction
$Δ H$ =enthalpy of the reaction.
From the above diagram,
$E_{a} = E_{a}^{'} + Δ H$
Thus, $E_{a} > Δ H$

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For an endothermic reaction, energy of activation is Ea and enthalpy of reaction is ΔH (both of these in kJ/mol). Minimum value of Ea will be:

For an endothermic reaction, energy of activation is $E_{a}$ and enthalpy of reaction is $Δ H$ (both of these in kJ/mol). Minimum value of $E_{a}$ will be: