The average Xe-F bond energy is 34 kcal/mol, first I.E of Xe is 279 kcal/mol, electron affinity of F is 85 kcal/mol & bond dissocitation energy of `F_(2)` si 38 kcal/mol. Then, the enthalpy change of the reaction
`XeF_(4)rarrXe^(+)+F^(-)+F_(2)+F` will be

The average Xe-F bond energy is 34Kcal//mol , first I.E . Of Xe is 279Kcal//mol , electron affinity of F is 85Kcal//mol . Then, the enthalpy chnage for the reaction XeF_(4)rarrXe^(+)+F^(-)+F_(2)+F will be

What is the bond enthalpy of Xe-F bond if Ionization energy of Xe = 279 kcal/mol B.E.(F-F) = 38 kcal/mol, electron affinity of F = 85 kcal//mol

The bond energy of H_(2) is 104.3 kcal mol^(-1) . If means that :

Calculate the enthalpy change for the following reaction: XeF_(4) rarr Xe^(o+) +F^(Theta) +F_(2) +F . The average Xe-F bond energy is 34 kcal mol^(-1) , first IE of Xe is 279 kcal mol^(-1), EA of F is 85 kcal mol^(-1) and bond dissociation enegry of F_(2) is 38 kcal mol^(-1)

Calculate the enthalpy change for the following reaction: XeF_(4) rarr Xe^(o+) +F^(Theta) +F_(2) +F . The average Xe-F bond energy is 34 kcal mol^(-1) , first IE of Xe is 279 kcal mol^(-1), EA of F is 85 kcal mol^(-1) and bond dissociation enegry of F_(2) is 38 kcal mol^(-1)

The enthalpy of formation of UF(g) is 22kcal mol^(-1) and that of U(g) is 128kcal mol^(-1) . The bond energy of the F-F bond is 37kcal mol^(-1) . The bond dissociation energy of UF(g) is (are):

The enthalpy of formation of UF(g) is 22kcal mol^(-1) and that of U(g) is 128kcal mol^(-1) . The bond energy of the F-F bond is 37kcal mol^(-1) . The bond dissociation energy of UF(g) is (are):

The heat of atomisation of PH_(3) is 228 K cal/mol and that os P_(2)H_(4) is 335 kCal/mol. The energy of P-P is (in kcal)