Ionisation energies of `CI^(-), CI` and `CI^(+)` are respectively (in kJ/mol):

CI_(2) is

CI_(2) is

Calculate free energy change for the reaction: H_(2)(g) + CI_(2)(g) rarr 2H-CI(g) by using the bond enegry and entropy data. Bond energies of H-H, CI-CI , and H-CI bonds are 435, 240 , and 430 kJ mol^(-1) , respectively. Standard entropies of H_(2),CI_(2) , and HCI are 130.59, 222.95 , and 186.68 J K^(-1) mol^(-1) , respectively.

Calculate free energy change for the reaction: H_(2)(g) + CI_(2)(g) rarr 2H-CI(g) by using the bond enegry and entropy data. Bond energies of H-H, CI-CI , and H-CI bonds are 435, 240 , and 430 kJ mol^(-1) , respectively. Standard entropies of H_(2),CI_(2) , and HCI are 130.59, 222.95 , and 186.68 J K^(-1) mol^(-1) , respectively.

Calculate the bond enthalpy of H-CI given that the bond enthalpies of H_(2) and CI_(2) are 435.4 and 242.8 kJ "mol"^(-1) respectively and enthalpy of formation of HCI(g) is -92.2 kJ mol

Calculate DeltaH of the reaction, H-underset(CI)underset(|)overset(H)overset(|)C-CI(g)rarrC(s) +2H(g) +2CI(g) Bond energy for C-H bond and C-CI bond are 400 kJ and 320kJ , respectively.