If bond enthalpy of `N_2`, `H_2` and NH bonds are 945 KJ/mol, 436 KJ/mol and 391 KJ/mol and enthalpy of vaporisation of `NH_3` is 405 KJ/mol. Calculate enthalpy of formation of `NH_3` [in KJ `mol^_1`]

Bond dissociation enthalpies of H_(2)(g) and N_(2)(g) are 436.0 kJ mol^(-1) and 941.8 kJ mol^(-1) , respectively, and ethalpy of formation of NH_(3)(g) is -46kJ mol^(-1) . What is the enthalpy fi atomisation of NH_(3)(g) ?. What is the avergae bond ethalpy of N-H bond?

Lattice energy of NaCl(s) is -790 kJ " mol"^(-1) and enthalpy of hydration is -785 kJ " mol"^(-1) . Calculate enthalpy of solution of NaCl(s).

If enthalpy of neutralisation of HCl by NaOH is -58.84 kJ/mol and by NH_4OH is -52.26 kJ/mol, then enthalpy of ionisation of NH_4OH is

If the enthalpy of formation of H_2O(l) is -x kj/mol and enthalpy of neutralization of HCl and NaOH is -y kj/mol then enthalpy of formation of OH^-1 ion (in kJ/mol) 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) )?

The enthalpy of formation of H_(2)O(l) is -280.70 kJ/mol and enthalpy of neutralisation of a strong acid and strong base is -56.70 kJ/mol. What is the enthalpy of formation of OH^(-) ions?

The bond energies of H - H and I - I bonds are 435 kJ mol^-1 and 150 kJ mol^-1 respectively. If DeltaH_f^o for HI is 26.5 kJ mol^-1 then bond enthalpy of H-I bond is

For Br_2(l) Enthalpy of atomisation = x kJ/mol, Bond dissociation enthalpy of bromine = y kJ/mole, then

Enthalpy of neutralization of HCl by NaOH is -57.1 J//mol and by NH_(4)OH is -51.1 KJ//mol . Calculate the enthalpy of dissociation of NH_(4)OH .

Lattice energy of NaCl_((s)) is -788kJ mol^(-1) and enthalpy of hydration is -784kJ mol^(-1) . Calculate the heat of solution of NaCl_((s)) .