The heat of formations for `CO_(2)(g),H_(2)O(l) and CH_(4)(g)` are -400 kJ `mol^(-1),-280" kJ "mol^(-1) and -70" kJ "mol^(-1)`, respectively. The heat of combustion of `CH_(4)` in kJ `mol^(-1)` is

The heat of formations for CO_(2)(g),H_(2)O(l) and CH_(4)(g) are -400kJ"mol"^(-1), -280kJ"mol"^(-1) and -70kJ"mol"^(-1) respectively. The heat of combustion of CH_(4) in kJ"mol"^(-1) is

The heats of formation of CO_(2(g)) , H_2O_((l)) and CH_(4(g)) are respectively –394 kJ mol^(-1), -286 kJ mol^(-1) and -76 kJ mol^(-1) . Calculate the heat of combustion of methane.

At 25^(@)C and 1 atm, heat of formation of C_(2)H_(4) (g), CO_(2)(g) and H_(2)O(l) are 52 " kJ mol"^(-1), -394 " kJ mol"^(-1) and -286 " kJ mol"^(-1) respectively. Calculate the heat of combustion of C_(2)H_(4)(g) .

The standard enthalpies fo formation of CO_(2) (g), H_(2) O (1) , and glucose (s) at 25^(@)C are - 400 kJ mol^(-1), - 300 kJ mol^(-) , and - 1300 kJ mol^(-1) , respectively. The standard enthalply of combustion per gram of glucose at 25^(@)C is

The standard enthalpies fo formation of CO_(2) (g), H_(2) O (1) , and glucose (s) at 25^(@)C are - 400 kJ mol^(-1), - 300 kJ mol^(-) , and - 1300 kJ mol^(-1) , respectively. The standard enthalply of combustion per gram of glucose at 25^(@)C is

At 25^(@)C temperature, the standard heat of formation of CH_(4)(g),CO_(2)(g) and H_(2)O(g) are -74.8 kJ*mol^(-1),-393.5kJ*mol^(-1)&-241.6kJ*mol^(-1) respectively. How much heat will be evolved during combustion of 1m^(3)CH_(4)(g) at 25^(@)C temperature and 1 atm pressure ? Consider CH_(4)(g) behaves like an ideal gas.

The standard enthalpies of formation of H_(2)O(l) and CO_(2)(g) are respectively -286" kJ mol"^(-1) and -394" kJ mol"^(-1) . If the standard heat of combustion of CH_(4)(g)" is "-891" kJ mol"^(-1) , then the standard enthalpy of formation of CH_(4)(g) is

Delta H_("combustion") of C _(6) H _(6) (l) . C(s) and H _(2) (g) are - 3000 kJ ,-390KJ mol^(-1) and - 290 kJ mol ^(-1) respectively. Hence heat of formation of benzene, is