Chemistry

Chemistry

Problem

For the reaction H2(g)+F2(g)→2HF(g)\mathrm{H_2(g) + F_2(g) \rightarrow 2HF(g)} the enthalpy change is ΔHrxn=−542 kJ mol−1\Delta H_{\text{rxn}} = -542\,\text{kJ\,mol}^{-1}. Given the average bond energies D(H ⁣− ⁣H)=436 kJ mol−1D(\mathrm{H\! -\! H}) = 436\,\text{kJ\,mol}^{-1} and D(F ⁣− ⁣F)=158 kJ mol−1D(\mathrm{F\! -\! F}) = 158\,\text{kJ\,mol}^{-1}, what is the average bond energy of the H ⁣− ⁣F\mathrm{H\! -\! F} bond? a) 560 kJ mol−1560\,\text{kJ\,mol}^{-1} b) 654 kJ mol−1654\,\text{kJ\,mol}^{-1} c) 568 kJ mol−1568\,\text{kJ\,mol}^{-1} d) 594 kJ mol−1594\,\text{kJ\,mol}^{-1}

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