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Answer :
The calculated bond energy for the C=C bond in ethene (C2H4) is 70.45 kcal. This value is obtained by considering the total bond breaking energy versus bond making energies, given the enthalpy of formation and other bond energies provided. None of the answer choices match this calculated value, indicating a potential error.
Explanation:
To determine the bond energy of the C=C bond, we can apply the concepts of bond energies and enthalpy of reaction. The enthalpy change (ΔH) for the formation of ethene (C₂H₄) is given as 12.5 kcal. The bond energies for atomisation of carbon and dihydrogen, as well as the bond energy of a carbon-hydrogen bond are provided. We use these energies to calculate the C=C bond energy as follows:
Bond energy for C₂H₄ formation is the sum of:
2 × C=C bond energy,
4 × C-H bond energy,
Bond energy for atomisation of 2 C atoms = 2 × 171 kcal,
Bond energy for formation of 2 H₂ molecules = 2 × 104.3 kcal.
The total energy for breaking the C₂H₄ molecule into atoms is the sum of the C=C bond energy and the energy of the four C-H bonds. This total must equal the atomisation energy plus the energy for forming H₂ molecules (since breaking H₂ gives the same energy but opposite sign). So, the equation is:
2 × C=C bond energy + 4 × 99.3 kcal = 2 × 171 kcal + 2 × 104.3 kcal - 12.5 kcal
Solving for the C=C bond energy:
2 × C=C bond energy = (2 × 171) + (2 × 104.3) - (4 × 99.3) - 12.5
2 × C=C bond energy = 550.6 - 397.2 - 12.5
2 × C=C bond energy = 140.9 kcal
C=C bond energy = 140.9 kcal / 2
C=C bond energy = 70.45 kcal
Since none of the provided choices match the calculated value of 70.45 kcal, there may be a mistake in the calculation or in the provided choices. The student should double-check their provided values and question prompt.
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