For an endothermic reaction, where `Delta H` represents the enthalpy of reaction in `kJ mol^(-1)`, the minimum value for the energy of activation will be

Options

A. less than `DeltaH`
B. zero
C. more than `DeltaH`
D. equal to `Delta H`

Explanation

For a reaction : `E_(a("forward"))=DeltaH+E_(a("backward"))` For endothermic reaction, `DeltaH`= positive thus `E_(a("backward")) gt DeltaH`