Chemistry

Chemistry

Problem

Using the average bond energies in the table, calculate the approximate enthalpy change, ΔH\Delta H, for the reaction below. CH4(g)+Cl2(g)→CH3Cl(g)+HCl(g)\text{CH}_{4}(g)+\text{Cl}_{2}(g)\rightarrow \text{CH}_{3}\text{Cl}(g)+\text{HCl}(g) Bond energies (kJ mol−1\text{kJ}\,\text{mol}^{-1}): C–H = 413C–Cl = 328H–Cl = 431Cl–Cl = 243\text{C–H}\,=\,413 \quad \text{C–Cl}\,=\,328 \quad \text{H–Cl}\,=\,431 \quad \text{Cl–Cl}\,=\,243 Which of the following is closest to the predicted ΔH\Delta H for the reaction? a) +103 kJ mol−1+103\,\text{kJ}\,\text{mol}^{-1} b) +328 kJ mol−1+328\,\text{kJ}\,\text{mol}^{-1} c) −103 kJ mol−1-103\,\text{kJ}\,\text{mol}^{-1} d) −346 kJ mol−1-346\,\text{kJ}\,\text{mol}^{-1}

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