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Hess' Law

Use the bond ...

Question

Use the bond energy data and calculate the enthalpy change for the above given reaction.
The bond energies of $C - H$ and $C - C l$ are $413$ and $328 k J {m o l}^{- 1}$ respectively.

A

1482 k J {m o l}^{- 1}

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B

- 1482 k J {m o l}^{- 1}

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C

2482 k J {m o l}^{- 1}

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D

- 2482 k J {m o l}^{- 1}

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Solution

The correct option is B $- 1482 k J {m o l}^{- 1}$
$Δ H = e n e r g y o f b o n d f o r m a t i o n o f r e a c t a n t - e n e r g y o f b o n d f o r m a t i o n o f p r o d u c t$
$Δ H = 0 - (413 + 413 + 328 + 328) = - 1482 K J m o l^{- 1}$

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Q. Using the bond enthalpy data given below, calculate the enthalpy of formation of acetone (g)
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C - C = 347.0 k J {m o l}^{- 1}

C = O = 728.0 k J {m o l}^{- 1}

O = O = 495.0 k J {m o l}^{- 1}

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Δ H_{s u b} C (s) = 718.4 k J {m o l}^{- 1}

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