When 2 moles of `C_(2)H_(6)(g)` are completely burnt `3120` kJ of heat is liberated. Calculate the enthyalpy of formation, of `C_(2)H_(6)(g)`. Given `Delta_(f)H` for `CO_(2)(g)` & `H_(2)O(l)` are `-395` & `-286` kJ respectively.

When 2mole of C_(2)H_(6) are completely burnt 3129kJ of heat is liberated. Calculate the heat of formation of C_(2)H_(6).Delta_(f)H^(Theta) for CO_(2) and H_(2)O are -395 and -286kJ , respectively.

When 2mole of C_(2)H_(6) are completely burnt -3129kJ of heat is liberated. Calculate the heat of formation of C_(2)H_(6).Delta_(f)H^(Theta) for CO_(2) and H_(2)O are -395 and -286kJ , respectively.

When 2mole of C_(2)H_(6) are completely burnt 3129kJ of heat is liberated. Calculate the heat of formation of C_(2)H_(6).Delta_(f)H^(Theta) for CO_(2) and H_(2)O are -395 and -286kJ , respectively.

The standard enthalpy of formation of octane (C_(8)H_(18)) is -250kJ //mol . Calculate the enthalpy of combustion of C_(8)H_(18) . The enthalpy of formation of CO_(2)(g) and H_(2)O(l) are -394 kJ//mol and -286kJ//mol respectively.

The standard enthalpy of formation of octane (C_(8)H_(18)) is -250kJ //mol . Calculate the enthalpy of combustion of C_(8)H_(18) . The enthalpy of formation of CO_(2)(g) and H_(2)O(l) are -394 kJ//mol and -286kJ//mol respectively.

Calculate Delta_(f)H^(@) for the reaction, CO_(2)(g) + H_(2)(g) to CO(g) + H_(2)O(g) Given that Delta_(f)H^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -393.5, -111.3 and -241.8 kJ mol^(-1) respectively.

Calculate the heat of formation of benzene given that the standard heat of combustion of benzene is - 3266 kJ and standard heat of formation of CO_(2)(g) and H_(2)O(l) are - 393.1 kJ and - 286 kJ respectively.

The heat of formation of H_(2)O_((l)) is -286.2 kJ. The heat of formation of H_(2)O_((g)) is likely to be