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 change for the following reaction is 368 kJ. Calculate the average O-F bond energy. OF_(2)(g)rarrO(g)+2F(g)

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):

Resonance energy of benzene is 36 kcal mol^(-1) . This means

The bond energy (in kcal mol^(-1)) of a C -C single bond is approximately

Calculate the enthalpy change for the reaction H_2(g) + 1/2 O_2(g) to H_2O (g) if the bond energies of H - H,O = O and O - H bonds are 104, 118 and 11 kcal mol^(-1) respectivley.

The bond energy (in kcal mol^(-1)) of a C -c single bond is approximately

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) .

From the following data, calculate the standard enthalpy of formation of propane Delta_(f)H^(Theta) CH_(4) = - 17 kcal mol^(-1) Delta_(f)H^(Theta)C_(2)H_(6) =- 24 kcal mol^(-1), BE (C-H) = 99 kcal mol^(-1) (C- C) = 84 kcal mol^(-1) .

An exothermic reaction, A rarr B , has an activation energy of "15 kcal mol"^(-1) and the energy of reaction is "5 kcal mol"^(-1) . The activation energy in "kcal mol"^(-1) for the reaction, BrarrA is

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