If the bond dissociation energies of `XY,X_(2)` and `Y_(2)(` all diatomic molecules `)` are in the ratio `1:1:0.5` and `Delta_(f)H` of `XY` is `-200 kJ mol^(-1)`. The bond dissociation energy of `X_(2)` will be `:`

If the bond dissociation energy of XY, x_ (2) AND y_(2) (all diatomic molecules) are in the ratio of 1 : 1 : 0.5 and Delta_(f)H for the formation of XY is - 200 kJ mol^(-1) . The bond dissociation energy of X_(2) will be :

Bond disociation enegry of XY,X_(2) and Y_(2) (all diatomic molecules) are in the ratio of 1: 1:0.5 and DeltaH_(f) of XY is -100 kJ mol^(-1) . The bond dissociation enegry of X_(2) is 100x . Find the value of x .

The bond dissociation energies of XY, X_2 and Y_2 (all diatomic molecules) are in the reaction 1:1:0:5 and Delta H_r for the formation of XY is -200 KJ mol^(-1) what will be the bond dissociation energy of X_2 ?

If the bond dissociation energies of XY , X_(2) and Y_(2) are in the ratio of 1:1:0.5 and DeltaH_(f) for the formation of Xy is -200 KJ//mol . The bond dissociation energy of X_(2) will be :-