Calculate `Delta_fH^(@) ("in" (kJ)/("mol"))` for `C_2H_6(g)`, if `Delta_cH^@` `[C("graphite")] = –393.5 (kJ)/(mol)`, `Delta_c H^@ [(H_2)g]= –286 (kJ)/(mol)` and `Delta_cH^@ [C_2H_6(g)]` = `–1560 (kJ)/(mol)`

Calculate the resonance energy of toluene (use Kekule structure from the following data C_(7)H_(8)(l) +9O_(2)(g) rarr 7CO_(2)(g) +4H_(2)O(l)+ DeltaH, DeltaH^(Theta) =- 3910 kJ mol^(-1) C_(7)H_(8)(l) rarr C_(7)H_(8)(g), DeltaH^(Theta) = 38.1 kJ mol^(-1) Delta_(f)H^(Theta) (water) =- 285.8 kJ mol^(-1) Delta_(f)H^(Theta) [CO_(2)(g)] =- 393.5 kJ mol^(-1) Heat of atomisation of H_(2)(g) = 436.0 kJ mol^(-1) Heat of sublimation of C(g) = 715.0 kJ mol^(-1) Bond energies of C-H, C-C , and C=C are 413.0, 345.6 , and 610.0 kJ mol^(-1) .

Calculate DeltaE° for the reaction CaC_2(S)+2H_2O(l) rarr Ca(OH)_2 (s)+C_2H_2(g) if DeltaH°_f( CaC_2) =-62.0(KJ/mol) DeltaH°_f(H_2O) =-286.0KJ/mol DeltaH°_f{Ca(OH)_2} =-986.0(KJ/mol) DeltaH°_f(C_2H_2) =+225.0(KJ/mol)

Calculate delta H° for the reaction , CaC_2(s) + 2H_2O(l) rarr Ca(OH)_2(s) + C_2H_2(g) , delta H°_(f(CaC_2)) = -62.0 kj/mol , delta H°_(f(H_2O)) = -286.0 kj/mol , delta H°_(f(CaOH_2)) = -986.0 kj/mol , delta H°_(f(C_2H_2)) = -227.0 kj/mol ,

Calculate the standard heat of formation of C_2H_5OH(l) from the following data: (a) C_2H_5OH (l) + 2O_2(g) to 2CO_2(g) + 3H_2O (l) , DeltaH^@ = - 1366.5 kJ (b) Delta_f H^@ [ CO_2] = -393.5 kJ mol^(-1), Delta_f H^@ [ H_2O(l)] = -285.5 kJ mol^(-1) .

Calculate the equilibrium constant for the following reaction at 298 K and 1 atm pressure.C(graphite)+H2O(l)=CO(g)+H2(g) Given : 'Delta_f H^@ , [H_2O (l)] = -286.0 kJ mol^(-1) , Delta_f H^@ [ CO (g)] = - 110.5 kJ mol^(-1) , DeltaS^@ at 298 K for the reaction =252.6 J k^(-1) mol^(-1) . Gas constant R = 8.31 Jk^(-1) mol^(-1) .

With the help of thermochemical equations given below, determine Delta_(r )H^(Θ) at 298 K for the following reaction: C("graphite")+2H_(2)(g) rarr CH_(4)(g),Delta_(r )H^(Θ) = ? C("graphite")+O_(2)(g) rarr CH_(2)(g), Delta_(r )H^(Θ) = -393.5 kJ mol^(-1) ...(1) H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l) , Delta_(r )H^(Θ) = -285.8 kJ mol^(-1) ...(2) CO_2(2)(g)+2H_(2)O(l) rarr CH_(4)(g)+2O_(2)(g) , Delta_(r )H^(Θ) = +890.3 kJ mol^(-1) ...(3)

Calculate standard free energy change from the free energy of formation data for the following reaction, C_(6)H_(6)(l)+(15)/(2)O_(2)(g)to 6CO_(2)(g)+3H_(2)O(g) . Delta_(f)G^(theta)[C_(6)H_(6)(l)]=172.8 kJ/mol Delta_(f)G^(theta)[CO_(2)(g)]=-394.4 kJ/mol Delta_(r )G^(theta)[H_(2)O(l)]=-228.6 kJ/mol

Methanol can be prepared synthetically by heating carbon monoxide and hydrogen gases under pressure in the presence of a catalyst. The reaction is CO(g) +2H_(2)(g) rarr CH_(3)OH(l) Determine the enthalpy of this reaction by an appropriate combinantion of the following data: a. C_(("graphite")) +(1)/(2)O_(2)(g) rarr CO(g), DeltaH^(Theta)=- 110.5kJ mol^(-1) b. C_(("graphite")) +O_(2)(g) rarr CO_(2)(g), DeltaH^(Theta) =- 393.5 kJ mol^(-1) c. H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(l), DeltaH^(Theta) =- 285.9kJ mol^(-1) d. CH_(3)OH(l) +(3)/(2)O_(2)(g)rarr CO_(2)(g) +2H_(2)O(l),DeltaH^(Theta) =- 726.6 kJ mol^(-1)

Calculate the EA of O atom to O^(2-) ion from the following data: i. Delta_(f)H^(ɵ)[MgO(s)] = -600 kJ mol^(-1) ii. Delta_(u)H^(ɵ) [MgO(s)] = -3860 kJ mol^(-1) iii. IE_(1) + IE_(2) of Mg(g) = 2170 kJ mol^(-1) iv. Delta_("diss")H^(ɵ) of Mg(s) = + 494 kJ mol^(-1) v. Delta_("sub")H^(ɵ) of Mg(s) = +150 kJ mol^(-1)

Calculate the enthalpy of combustion of benzene (l) on the basis of the following data: a. Resonance energy of benzene (l) =- 152 kJ// mol b. Enthalpy of hydrogenation of cyclohexene (l) =- 119 kJ//mol c. Delta_(f)H^(Theta)C_(6)H_(12)(l) =- 156 kJ mol^(-1) d. Delta_(f)H^(Theta) of H_(2)O(l) =- 285.8 kJ mol^(-1) e. Delta_(f)H^(Theta)of CO_(2)(g) =- 393.5 kJ mol^(-1)