`Delta H^(0)` for a reaction `F_(2)+2HCl rarr2HF+Cl_(2)` is given as `-352.8kJ`. `Delta H_(f)^(0)` for `HF` is `-268.3kJmol^(-1)`, then `Delta H_(f)^(0)` of `HCl` would be

Calorific value of H_2 is -143KJ g^(-1) . Hence, Delta H_(f)^(@) of H_2O is:

Calculate DeltaG^@ for the reaction 2HCl (g) + F_2(g) to 2HF (g) + Cl_2(g) at 25^@C at Given : Delta_f G^@ [ HCl (g)] = -95.30 kJ mol^(-1) . Delta_fG^@ [ HF(g)] = -273 kJ mol^(-1) . Also calculate the equilibrium constant the reacton at 25^@C . Given, gas constant R = 8.314 JK^(-1) mol^(-1) .

For the reaction PCI _(3) (g) + CI_(2)(g) rightarrow PCI_(5)(g), Delta H = -x kJ If the Delta H_(f)^(@)"PCI"_(3) is -y kJ, what is Delta H_(f)^(@)PCI_(5) ?

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 ,

The bond enthalpies of H-H and Cl-Cl are 430 and 242 kJ mol^(-1) , respectively. If DeltaH_(f) (HCl) is -91 kJmol^(-1) the bond enthalpy of HCl would be

The enthalpy change for the combustion of N_(2)H_(4)(l) (Hydrazine) is -622.2 kJ mol^(-1) . The products are N_(2)(g) and H_(2)O(l) . If Delta_(f)H^(Theta) for H_(2)O(l) is -285.8 kJ mol^(-1) . The Delta_(f)H^(Theta) for hydrazine is

Calculate Deltah for the eaction BaCO_(3)(s)+2HCI(aq) rarr BaCI_(2)(aq)+CO_(2)(g)+H_(2)O(l) Delta_(f)H^(Theta) (BaCO_(3)) =- 290.8 kcal mol^(-1), Delta_(f)H^(Theta) (H^(o+)) =0 Delta_(f)H^(Theta) (Ba^(++)) = - 128.67 kcal mol^(-1) , Delta_(f)H^(Theta)(CO_(2)) =- 94.05 kcal mol^(-1) , Delta_(f)H^(Theta) (H_(2)O) =- 68.32 kcal mol^(-1)

Find Delta H_(f)^(@) of Fe_(2)O_(3)(s) if the standard heat reaction Fe_(2)O_(3)(s)+3CO(g)rarr 2Fe(s)+3CO_(2)(g) is -6.6 kcal. Given Delta H_(f)^(@)CO(g)=-26.4 kcal. Delta H_(f)^(@)CO_(2)(g)=-94 kcal .

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 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) .