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[" Bond dissociation energy of "XY,X_(2)," and "Y_(2)" (all "],[" diatomic molecules ) are in the ratio of "1:1:0.5" and "],[Delta H_(f)" of "XY" is "-100kJmol^(-1)" .The bond dissociation "],[" energy of "X_(2)" is "100x" Find the value of "x" ."],[" Numeric Answer: "]

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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 .

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 :

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 ?