From the following bond energies:
H−H bond energy: 431.37 kJ mol⁻¹
C−C bond energy: 606.10 kJ mol⁻¹
C−H bond energy: 336.49 kJ mol⁻¹
Enthalpy for the reaction:
H−H
|
C = C + H−H → H−C−C−H
|
H H H H
will be:

Question

Accepted Answer

−243.6 kJ mol⁻¹. The reaction involves breaking one H−H bond and one C=C bond, and forming two C−H bonds and one C−C bond. Using bond energies: ΔH = [431.37 + 606.10] − [2(336.49) + 606.10] = −243.6 kJ mol⁻¹.

From the following bond energies: H−H bond energy: 431.37 kJ mol⁻¹ C−C bond energy: 606.10 kJ mol⁻¹ C−H bond energy: 336.49 kJ mol⁻¹ Enthalpy for the reaction: H−H | C = C + H−H → H−C−C−H | H H H H will be:

Solution

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