Calculate the lattice energy of `NaCI` crystal from the following data by the use of Born-Haber cycle. Sublimation energy of `Na = 26 kcal//g`atom, dissociation energy of `CI_(2) = 54 kcal//"mole"`, ionisation energy of `Na(g) = 117 kcal//"mol"`, electron affinity for `CI(g) = 84 kcal//g` atom, heat of formation of `NaCI =- 99 kcal//"mole"`.

Calculate the lattice energy of formation of NaCl from the following data : Na_((s)) +1//2Cl_(2(g)) to NaCl_((s)) Delta H_(f) -411.3 KJ.mol^(-1) Heat of sublimation of Na_((s)) = 108 . 7 kJ mol ^(-1) Ionisation energy of Na_((g)) = 49.5.0 kJ mol^(-1) Dissociation energy of Cl_(2(g)) = 244 kJ mol^(-1) Electron affinity of Cl_((g)) = - 349 . 0 kJ mol^(-1)

For NaCl , lattice energy = - 186 kcal//mol , the solvation energy of Na^(+) and Cl are -97 and -85 kcal//"mole" respectively. Therefore for NaCl (s)

Find the electron affinity of chlorine from the following data. Enthalpy of formation of LiCI is -97.5 kcal mol^(-1) , lattice energy of LiCI =- 197.7 kcal mol^(-1) . Dissociation energy of chlirine is 57.6 kcal mol^(-1) , sublimation enthalpy of lithium =+ 38.3 kcal mol^(-1) , ionisation energy of lithium =123.8 kcal mol^(-1) .

Find the electron affinity of chlorine from the following data. Enthalpy of formation of LiCI is -97.5 kcal mol^(-1) , lattice energy of LiCI =- 197.7 kcal mol^(-1) . Dissociation energy of chlirine is 57.6 kcal mol^(-1) , sublimation enthalpy of lithium =+ 38.3 kcal mol^(-1) , ionisation energy of lithium =123.8 kcal mol^(-1) .

The dissociation energy of CH_(4)(g) is 360 kcal mol^(-1) and that of C_(2)H_(6)(g) is 620 kcal mol^(-1) . The C-C bond energy

The dissociation energy of CH_(4)(g) is 360 kcal mol^(-1) and that of C_(2)H_(6)(g) is 620 kcal mol^(-1) . The C-C bond energy

Prove that the formation of NaCI_(2) is highly endothermic and energetically unfavorable from the following data using Born-Haber Cycle {:("Heat of sublimation of"Na,=,109kJ//mol),(1^(st)IE of Na,=,494 kJ//mol),(1^(st)IE of Na^(+),=,4563 kJ//mol),("Bond Energy of" CI_(2),=,242 kJ//mol),("Electron gain enthalpy of"CI,=,-347 kJ//mol),("Lattice energy of" NaCI_(2),=,2560 kJ//mol):}

Calculate the heat of formation of benzene from the following data, assuming no resonance. Bond energies : C-C=83 kcal, C=C=140 Kcal, C-H=99 kcal {:("Heat of atomisation of ",C-170 9 kcal,,,),("Heat of atomisation of",H=6xx52.1 kcal,,,):}