Statement I : Negative electron gain enthalpy of chlorine is greater than negative electron gain enthalpy of bromine

Statement II : ${\mathrm{Cl}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}\to {\mathrm{Cl}}_{\left(\mathrm{g}\right)}^{-}$   is  thermodynamically more favourable than${\mathrm{Br}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}\to {\mathrm{Br}}_{\left(\mathrm{g}\right)}^{-}$

 

negative electron gain enthalpy of chlorine is more than negative electron gain enthalpy of bromine, chloride ion is readily formed than bromide ion . Both statements are correct but statement I explains statement II but not statement II explains statement I.