If bond enthalpies Of `N-=N,H-Hand N-H` bonds are `x_(1),x_(2)and x_(3)` respectively ,`DeltaH_(f)^(@)`for `NH_(3)` will be :

Bond energies of N -= N H-H, N - H are respectively x_1 , x_2, x and X_3 kJ mol^(-1) . Hence, DeltaH_(f)^(@)(NH_3) is:

Bond energies of N -= N H-H, N - H are respectively x_1 , x_2, x and X_3 kJ mol^(-1) . Hence, DeltaH_(f)^(@)(NH_3) is:

The bond enthalpies of H-H and CI-CI are 430 and 242 kJ mol^(-1) , respectively. If DeltaH_(f) (HCI) is -91 kJmol^(-1) the bond enthalpy of HCI would be

The bond enthalpies of H-H and Cl-Cl are 430 and 242 kJ mol^(-1) , respectively. If DeltaH_(f) (HCl) is -91 kJmol^(-1) the bond enthalpy of HCl would be

Given that bond energies of N=N,H-H and N-H bonds as 945, 436 and 391 kJ/ mol respectively ,the enthalpy of the reaction N_(2)(g)+3H_(2)(g)+to2NH_(3)(g), is

Heat of formation of 2 mol of NH_(3)(g) is =90 kJ , bond energies of H-H and N-H bonds are 435kJ and 390 kJ mol^(-1) , respectively. The value of the bond enegry of N-=N will be

Heat of formation of 2 mol of NH_(3)(g) is =90 kJ , bond energies of H-H and N-H bonds are 435kJ and 390 kJ mol^(-1) , respectively. The value of the bond enegry of N-=N will be