If bond enthalpy of C − C and C = C are 348 kJ / mole and 615 kJ / mole respectively then calculate enthalpy change (in kJ / mole) which occurs during the isomerisation of cyclopropane (g) into propen

Question

If bond enthalpy of C − C and C = C are 348 kJ / mole and 615 kJ / mole respectively then calculate enthalpy change (in kJ / mole) which occurs during the isomerisation of cyclopropane (g) into propene (g)

TestHub · Accepted Answer

Concepts: Enthalpy change from bond energies, ring strain.

$Δ H = \sum (b o n d s b ro k e n) - \sum (b o n d s f or m e d)$

$Δ H = (6 \times C - H + 3 \times C - C) - (6 \times C - H + 1 \times C - C + 1 \times C = C)$ $Δ H = 2 \times C - C - C = C$

$Δ H = 2 (348) - 615 = 696 - 615 = 81 k J / m o l$

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