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

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

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

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

The heat of formation of C_(2)H_(5)OH(l) is -66Kcal//mol . The heat of combustion of CH_(3)OCH_(3)(g) is -348Kcal//mol , DeltaH_(f) for H_(2)O and CO_(2) are -68Kcal//mol and -94Kcal//mol . Respectively. Then, the DeltaH for the isomerisation reaction C_(2)H_(5)OH(l)rarrCH_(3)OCH_(3)(g) , and DeltaE for the same are at T=25^(@)C

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):