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 `DeltaH`

Answer

c

Explanation

We know that , `DeltaH=E_(f)-E_(b)`
where , `E_(b)&E_(f)=` activation energy for backward and forward respectively .
Thus , `E_(f)=DeltaH+E_(b)` , means `E_(F)gtDeltaH` .