Chemistry

Chemistry

Problem

The reaction 2 AB(g)+C2(g)→2 AC(g)+B2(g)\mathrm{2\,AB(g) + C_2(g) \rightarrow 2\,AC(g) + B_2(g)} has an experimentally determined enthalpy change of  ⁣−120 kJ\!-120\,\text{kJ} for the equation as written. Using the average bond energies D(A ⁣− ⁣B)=250 kJ mol−1D(\mathrm{A\! -\! B}) = 250\,\text{kJ\,mol}^{-1}, D(A ⁣− ⁣C)=330 kJ mol−1D(\mathrm{A\! -\! C}) = 330\,\text{kJ\,mol}^{-1}, and D(C ⁣− ⁣C)=348 kJ mol−1D(\mathrm{C\! -\! C}) = 348\,\text{kJ\,mol}^{-1}, determine the average bond energy of the B ⁣− ⁣B\mathrm{B\! -\! B} bond in B2(g)\mathrm{B_2(g)}. a) 348 kJ mol−1348\,\text{kJ\,mol}^{-1} b) 154 kJ mol−1154\,\text{kJ\,mol}^{-1} c) 308 kJ mol−1308\,\text{kJ\,mol}^{-1} d) 298 kJ mol−1298\,\text{kJ\,mol}^{-1}

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