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The combustion of 1 mole of benzene take...

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

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To calculate the standard enthalpy of formation (Δ_fH°) of benzene (C₆H₆), we will use Hess's law, which states that the total enthalpy change during a chemical reaction is the same, regardless of the number of steps in the reaction. ### Step-by-Step Solution: 1. **Write the combustion reaction of benzene:** The balanced equation for the combustion of benzene is: \[ C_6H_6 (l) + \frac{15}{2} O_2 (g) \rightarrow 6 CO_2 (g) + 3 H_2O (l) ...
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The combustion of 1 mole of benzene takes placeat 298K and 1 atm. After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0kJ of heat is liberated. Calculate the standard enthalpy of formation, Delta _(f) H^(@) of benzene. Standard enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5kJ mol^(-1) and -258.83kJ 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.

Knowledge Check

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

    A
    -5200 KJ/mol
    B
    -5726 KJ/mol
    C
    -5476 KJ/mol
    D
    -5310 KJ/mol

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    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.

    Calculate the enthalpy of formation of acetic acid (CH_(3)COOH) if its enthalpy of combustion is 867 kJ mol^(-1) .The enthalpies of fromation of CO_(2)(g) and H_(2)O(l) are -393.5 and -285.9 kJ mol^(-1) respectively.

    The combustion of 1 mol of benzene takes place at 298 K. After combustion CO_(2) and H_(2)O are formed and 3267 kJ mol^(-1) of heat is liberated. Calculate Delta_(f) H^(0) (C_(6)H_(6)) . Given: Delta_(f) H^(0) (CO_(2)) = -286kJ mol^(-1), Delta_(f) H^(0) (H_(2)O) = - 393 kJ mol^(-1)

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