Chemistry

Chemistry

Problem

Consider the chlorination reaction CH4(g)+Cl2(g)  →  CH3Cl(g)+HCl(g)\mathrm{CH_4(g)+Cl_2(g)\;\rightarrow\;CH_3Cl(g)+HCl(g)} Average bond energies (kJ mol−1^{-1}): C–H = 413; Cl–Cl = 243; C–Cl = 328; H–Cl = 431. What is the enthalpy change per mole of CH3Cl\mathrm{CH_3Cl} produced? a) +103 kJ mol−1+103\ \text{kJ\,mol}^{-1} b) −346 kJ mol−1-346\ \text{kJ\,mol}^{-1} c) −103 kJ mol−1-103\ \text{kJ\,mol}^{-1} d) +225 kJ mol−1+225\ \text{kJ\,mol}^{-1}

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