The combustion of one mole of benzene takes place at 298 K and 1 atm. After combustion, `CO_(2)(g) and H_(2)O (1)` are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation, `Delta_(f)H^(Ө)` of benzene. Standard enthalpies of formation of
`CO_(2)(g) and H_(2)O(1)` are -393.5kJ `"mol"^(-1)` and -285.83 kJ `"mol"^(-1)` respectively.

The combustion of 1 mole of benzene takes place at 298K and 1 atm. After combustion, CO_(2(g)) and H_(2)O_((l)) are produced and 3267.0 KJ of heat is liberated. Calculate the standard enthalpy of formation, Delta_(f)H^(0) of benene. Standard enthalpies of formation of CO_(2(g))andH_(2)O_((l)) are -393.5 KJ mol^(-1) and - 285.83 KJ mol^(-1) respectively

The combustion of one mole of benzene takes place at 298 and 1 atm. After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation. triangle_f H^@ benzene. Standard enthalpies of formation of CO_2(g) and H_20(l) are -393,5 kJ mol ""^(-1) and "-285.83 kJ mol"^(-1) respectively.

The combusition of 1 mol of benzene (C_(6) H_(6)) takes place at 298 K and 1 bar pressure. After combustion, CO_(2) (g) and H_(2) O (1) are produced and 3267 kJ of heat is liberated. Calculate the standard enthaply of formation, Delta_(f) H^(@) of benzene. Standard enthapies of formation of CO_(2) (g) and H_(2) O (1) are - 393.5 kJ mol^(-1) and - 258.83 kJ mol^(-1) , respectively. Strategy : Apply Eq. the mathematical form of Hesis's law, to the combustion reaction of 1 mol of benzene. Remember Delta_(f) H^(@) for O_(2) (g) is zero by convention. We are give Delta_(1) H^(@) and Delta_(f) H^(@) values for all substance except C_(6) H_(6) (1) . We can solve for this unknown.

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

The combustion of butane (C_(4)H_(10)) is exothermic by 2878.7 kJ "mol"^(-1) .Calculate the standard enthalpy of formation of butane given that the standard enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5 kJ "mol"^(-1) and -285.8 kJ "mol"^(-1) respectively.

Calculate the standard enthalpy of combustion of CH_(4) , it standard enthalpies of formation of CH_(4(g)),H_(2)O_((l)), and CO_(2(g)) are -74.81kJ mol^(-1), -285.83kJ mol^(-1) and -393.51kJ mol^(-1) respectively.

Calculate the standard enthalpy of formation of propane (C_(3)H_(8)) if its enthalpy of combustion is -2220.2 kJ "mol"^(-1) .The enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5 and -285.8 kJ "mol"^(-1) respectively.