91Ó°ÊÓ

In Appendix C, we can find the standard enthalpies of formation for acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\). The values are: - Standard enthalpy of formation of acetylene: \(\Delta H_f^{⦵}(\mathrm{C}_{2} \mathrm{H}_{2}) = 226.7 \,\mathrm{kJ/mol}\) - Standard enthalpy of formation of benzene: \(\Delta H_f^{⦵}(\mathrm{C}_{6} \mathrm{H}_{6}) = 49.0 \,\mathrm{kJ/mol}\)

To determine the enthalpy change for the given reaction, we will use the following equation: \(\Delta H_{rxn}^{⦵} = \sum n_p \Delta H_f^{⦵}(products) - \sum n_r \Delta H_f^{⦵}(reactants)\) where \(\Delta H_{rxn}^{⦵}\) is the standard enthalpy change for the reaction, \(\Delta H_f^{⦵}(products)\) is the standard enthalpy of formation of the products, \(\Delta H_f^{⦵}(reactants)\) is the standard enthalpy of formation of the reactants, \(n_p\) is the stoichiometric coefficient of product and \(n_r\) is the stoichiometric coefficient of reactant. For our reaction, \(3 \mathrm{C}_{2} \mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{6}(l)\): \(\Delta H_{rxn}^{⦵} = (1) \Delta H_f^{⦵}(\mathrm{C}_{6} \mathrm{H}_{6}) - (3) \Delta H_f^{⦵}(\mathrm{C}_{2} \mathrm{H}_{2})\) Substituting the values of standard enthalpies of formation from Step 1: \(\Delta H_{rxn}^{⦵} = (1)(49.0 \,\mathrm{kJ/mol}) - (3)(226.7 \,\mathrm{kJ/mol})\)

Perform the calculation: \(\Delta H_{rxn}^{⦵} = 49.0 \,\mathrm{kJ/mol} - 680.1 \,\mathrm{kJ/mol} = -631.1 \,\mathrm{kJ/mol}\) The standard enthalpy change for the reaction \(3 \mathrm{C}_{2} \mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{6}(l)\) is \(-631.1 \,\mathrm{kJ/mol}\).