Calculate the bond energy of O-H bond in `H_(2)O(g)` at the standard state from the following data:
(1) `H_(2)(g) to 2H(g),DeltaH^(0)=436kJ*mol^(-1)`
(2) `(1)/(2)O_(2)(g)toO(g),DeltaH^(0)=249k*mol^(-1)`
(3) `H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(g),DeltaH_(f)^(0)[H_(2)O(g)]=-241.8kJ*mol^(-1)`.

Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: (1) CH_(3)OH(l)+(3)/(2)O_(2)(g)toCO_(2)(g)+2H_(2)O(l),Delta_(r)H^(0)=-726kJ*mol^(-1) (2) C(s)+O_(2)(g) to CO_(2)(g),Delta_(c)H^(0)=-393kJ*mol^(-1) (3) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),Delta_(f)H^(0)=-286kJ*mol^(-1) .

Diborane [B_(2)H_(6)(g)] is used as a very effective fuel for rockets. Calculate the heat of combustion of diborane for the following reaction: B_(2)H_(6)(g)+3O_(2)(g)toB_(2)O_(3)(g)+3H_(2)O(g) Given: (1) 2B(s)+(3)/(2)O_(2)(g)toB_(2)O_(3) (s),DeltaH^(0)=-1273kJ*mol^(-1) (2) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),DeltaH^(0)=-285.8kJ*mol^(-1) . (3) H_(2)O(l)toH_(2)O(g),DeltaH^(0)=+44kJ*mol^(-1) (4) 2B(s)+3H_(2)(g) to B_(2)H_(6)(g),DeltaH^(0)=+36kJ*mol^(-1) .

Comment on the thermodynamic stability of NO(g). Given: (1)/(2)N_(2)(g)+(1)/(2)O_(2)(g)toNO(g),Delta_(r)H^(0)=90kJ*mol^(-1),NO(g)+(1)/(2)O_(2)(g)toNO_(2)g,Delta_(r)H^(0)=-74kJ*mol^(-1) .

Given: C(graphite, s) +O_(2)(g)toCO_(2)(g),DeltaH^(0)=x_(1) C(graphite, s) +(1)/(2)O_(2)(g) to CO(g),DeltaH^(0)=x_(2) CO(g)+(1)/(2)O_(2)(g) to CO_(2)(g),DeltaH^(0)=x_(3) Express x_(3) in terms of x_(1) and x_(2) .

Calculate the enthalpy of formation of liquid ethyl alcohol from the following data. C_(2)H_(5)OH(l)+3O_(2)(g)to2CO_(2)(g)+3H_(2)O(l),DeltaH=-1368kJ C(s)+O_(2)(g)toCO_(2)(g),DeltaH=-393kJ H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),DeltaH=-287kJ .

DeltaH value for the given reactions at 25^(@)C are- C_(3)H_(8)(g)to3C(s)+4H_(2)(g),DeltaH^(0)=103.8kJ*mol^(-1) 2H_(2)(g)+O_(2)(g) to 2H_(2)O(l),DeltaH^(0)=-571.6kJ*mol^(-1) C_(2)H_(6)(g)+(7)/(2)O_(2)(g)to2CO_(2)(g)+3H_(2)O(l),DeltaH^(0)=-1560kJ*mol^(-1) CH_(4)(g)+2O_(2)(g) to CO_(2)(g)+2H_(2)O(l),DeltaH^(0)=-890kJ*mol^(-1) C(s)+O_(2)(g) to CO_(2)(g),DeltaH^(0)=-393.5kJ*mol^(-1) Calculate DeltaH^(0) for the reaction at 25^(@)C C_(3)H_(8)(g)+H_(2)(g)toC_(2)H_(6)(g)+CH_(4)(g)

Calculate the standard enthalpy of formation of C_(6)H_(6)(l) at 25^(@)C temperature using the given data: C_(6)H_(6)(l)+(15)/(2)O_(2)(g) to 6CO_(2)(g)+3H_(2)O(l),DeltaH^(0)=-781kcal H_(2)(g)+(1)/(2)O_(2)(g) to H_(2)O(l),DeltaH^(0)=-68.32kcal C (s, graphite) +O_(2)(g)toCO_(2)(g),DeltaH^(0)=-94.04 kcal .

Given that (at 25^(@)C) : (1)/(2)H_(2)(g)+(1)/(2)O_(2)(g) to OH(g), Delta H^(0)= 38.95 " kJ mol"^(-1) H_(2)(g)+(1)/(2)O_(2)(g) to H_(2)O (g), Delta H^(0) = -241.8 " kJ mol"^(-1) H_(2)(g) to 2H(g), Delta H^(0)= 436.0 " kJ mol"^(-1) O_(2)(g) to 2O (g), Delta H^(0)= 498.3 " kJ mol"^(-1) Calculate Delta H^(0) for the following reaction - (a) OH(g) to H(g)+O(g) (b) H_(2)O(g) to 2H(g)+O(g)