Considering the parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy, compare the oxidising power of F₂ and CI₂.

The electrode potential of F₂ (+ 2.87 V) is much higher that that of Cl₂ (+ 1.36 V), therefore, F₂ is a much stronger oxidising agent than Cl₂. Now, electrode potential depends upon three factors : 

(i) bond dissociation energy,

(ii) electron gain enthalpy and

(iii) hydration energy. Although electron gain enthalpy of fluorine is less negative (–349 kJ mol^–1), the bond dissociation energy of F—F bond is much lower (158.8 kJ mol^–1) than that of Cl—Cl bond (242.6 kJ mol^–1), and hydration energy of F– ion (515 kJ mol^–1) is much higher than that of Cl^– ion (381 kJ mol^–1). 

The later two factor more than compensate the less negative electron gain enthalpy of F₂. As a result, electrode potential of F₂ is higher than that of Cl₂ and 

Hence, F₂ is a much stronger oxidising agent than Cl₂.