16. (1pt.) Use bond enthalpy data to estimate the heat of reaction for the following reaction. $CH_4(g) + 3 Cl_2(g) \rightarrow CHCl_3(g) + 3 HCl(g)$ Bond Enthalpies C-H: 413kJ/mol Cl-Cl: 242kJ/mol C-Cl: 328kJ/mol H-Cl: 431kJ/mol
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Use the bond enthalpies in the table below to calculate ΔrxnH° (in kJ.mol-1) for the following reaction: C2H4(g) + Cl2(g) → ClCH2CH2Cl(g) Bond | Bond Enthalpy (kJ/mol) C-H | 413 C-C | 348 C=C | 614 C-Cl | 328 Cl-Cl | 242
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Calculate the enthalpy for the following reaction using the given bond energies $(\mathrm{kJ} / \mathrm{mol}):$ $(C-H=414 ; H-O=463 ; H-C l=431, C-C l=326 ; C-O=335)$ $\mathrm{CH}_{3}-\mathrm{OH}(g)+\mathrm{HCl}(g) \longrightarrow \mathrm{CH}_{3}-\mathrm{Cl}(g)+\mathrm{H}_{2} \mathrm{O}(g)$ (a) $-23 \mathrm{~kJ} / \mathrm{mol}$ (b) $-42 \mathrm{~kJ} / \mathrm{mol}$ (c) $-59 \mathrm{~kJ} / \mathrm{mol}$ (d) $-511 \mathrm{~kJ} / \mathrm{mol}$
Calculate the enthalpy of reaction, in kJ, for the chemical equation, C3H8 (g) + 2 Cl2 (g) --> C3H6Cl2 (g) + 2 HCl (g) using the bond dissociation energies: Bond of Interest Bond Enthalpy (in kJ/mol) C-H 414 C-C 347 Cl-Cl 243 C-Cl 339 H-Cl 431 The corresponding Lewis structures for the compounds are:
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