The bond dissociation energies of gaseous `H_(2),C1_(2)`, and `HC1` are `100, 50`, and `100 kcal mol^(-1)`, respectively. Calculate the enthalpy of formation of `HC1(g)`.

The bond dissociation energy of gaseous H_(2),Cl_(2) and HCl are 104,58 and 103 kcal mol^(-1) respecitvely. Calculate the enthalpy of formation for HCl gas.

The bond dissociation energy of gaseous H_(2), Cl_(2) and HCl are 104, 58 and 103 kcal mol^(-1) respectively. The enthalpy of formation for HCl gas will be

The bond dissociation energy of gaseous H_(2),Cl_(2) and HCl are 104,58,103 kcal mol^(-1) respectively. The enthalpy of formation for HCl gas will be :

Bond energies of H_(2), Cl_(2) and HCI are respectively 104, 58 and 100 kcal mol^(-1) calculate Pauling's electronegativivy of chlorine.

Bond dissociation enthalpy of H_(2),Cl_(2) and HCl are 434,242 and 431kJ mol^(-1) respectively. Enthalpy of formation of HCl is :

Bond dissociation enthalpy of H_(2) , Cl_(2) and HCl are 434, 242 and 431KJmol^(-1) respectively. Enthalpy of formation of HCl is

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) )?