If the enthalpy of formation and enthalpy of solution of HCl (g) are-92.3kj /mol and -75.14kJ/mol respectively then find the enthalpy of `Cl^(-)`(aq):

Lattice enthalpy and enthalpy of solution of NaCl are 788 kJ"mol"^(-1) and 4kJ"mol"^(-1) respectively. The hydration enthalpy of NaCl is

Lattice enthalpy and enthalpy of solution of NaCl are 788 kJ"mol"^(-1) and 4kJ"mol"^(-1) respectively. The hydration enthalpy of NaCl is

If the enthalpy of formation of HCl (g) and Cl^(-) (aq) are -92.3 kJ/mole and -167.44 kJ/mol, find the enthalpy of solution of hydrogen chloride gas.

The standard enthalpies of formation of HCl(g), H(g) and Cl(g) are -92.2 , 217.7 and 121.4 kJ mol^(-1) respectively. The bond dissociation enthalpy of HCl is :

The enthalpy of solution , sodium and sodium oxide in large volume of water , are -18KJ/mole and -238KJ/mol, respectively . If the enthalpy of formation of water is -286 KJ/mol, then what is the enthalpy of formation of sodium oxide ? All the enthalpies are at 298K and 1 bar pressure. [Given : reaction involved are 2Na(s)+2H_(2)O(l)to 2NaOH(aq)+H_(2)(g) Na_(2)O(s)+H_(2)O(l)to2NaOH(aq)

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

Enthalpy of formation of HF and HCI are -161 kJ mol^-1 and -92kJ mol^-1 respectively. Which of the following statements is incorrect?