the bond enthalpy of `H_(2)(g)` is 436 ` kJ "mol"^(-1)` and that of `N_(2)(g)` is 941.3 `kJ"mol"^(-1)`. Calculate the average bond enthalpy of ann N-H bond in ammonia, `Delta_(t)^(@)(NH_(3)) =-46 kJ "mol"^(-1)`

The standard enthalpy of formation of NH_(3) is -46.0 kJ mol^(-1) . If the enthalpy of formation of H_(2) from its atoms is -436 kJ mol^(-1) and that of N_(2) is -7112kJ mol^(-1) , the average bond enthalpy of N-H bond in NH_(3) is :-

The standard enthalpy of formation of NH_(3) is - 46.0 kJ mol^(-1) . If the enthalpy of formation of H_(2) from its atoms is - 436 kJ mol^(-1) and that of N_(2) is - 712 kJ mol^(-1) , the average bond enthalpy of N - H bond is NH_(3) is

The standard enthalpy of formation of NH_(3) is -46.0KJ mol^(-1) . If the enthalpy of formation of H_(2) from its atoms is -436KJ mol^(-1) and that of N_(2) is -712KJ mol^(-1) , the average bond enthalpy of N-H bond in NH_(3) is

The bond energy of H_(2(g)) is 436kJ/mole. The bond enthalpy of N_(2(g)) is 941.3 kJ/mole. What is the bond enthalpy of N - H if NH_3 formation energy is -46.0 kJ/mole ?

Bond dissociation enthalpies of H_(2(g)) and N_(2(g)) are "426.0 kJ mol"^(-1) and "941.8 kJ mol"^(-1) , respectively, and enthalpy of formation of NH_(3(g))" is "-"46 kJ mol"^(-1) . What are the enthalpy of atomisation of NH_(3(g)) and the average bond enthalpy of N-H bond respectively ( in kJ "mol"^(-1) )?