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

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

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

Calorific value of ethane, in k J/g if for the reaction 2C_(2)H_(6) + 7O_(2) rightarrow 4CO_(2) + 6 H_(2)O, Delta H = -745.6 kcal

Calorific value of ethane, in k J/g if for the reaction 2C_(2)H_(6) + 7O_(2) rightarrow 4CO_(2) + 6 H_(2)O, Delta H = -745.6 kcal

Calculate Delta_(r)H^(@) for the reaction : Given Delta_(f)H^(@) values : 2H_(2)S(g) + 3O_2to 2H_(2)O(l) + 2SO_(2)(g) Given Delta_(f)H^(@) values : H_(2)S(g) = -20.60 , H_(2)O(l) = -285.83, SO_(2)(g) = -296.83 kJ "mol"^(-1)

Calculate the heat of reaction of the following reaction : CO_(2)(g) + H_(2)(g) rarr CO(g) + H_(2)O(g) Given that the Delta_(f)H^(@) of CO(g) = -110.5 kJ, Delta_(f)H^(@) of CO_(2)(g) = -393.8 kJ , Delta_(f)H^(@) of H_(2)O(g) = -241.8 kJ respectively