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Heat Capacity

Calculate the...

Question

Calculate the $Δ H$ of the reaction given (figure).
Bond energy for $C - H$ bond and $C - C l$ bond are $415 k J$ and $326 k J$ respectively.

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Solution

$Δ H =$ Sum of bond energies of reactants $-$ Sum of bond energies of products
$= [2 \times (C - H) + 2 \times (C - C l)] - 0$ (all the products are free atoms)
$= 2 \times 415 + 2 \times 326$
$= 830 + 652 = 1482 k J$

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Q. Calculate the

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H of the reaction

H - H | C | C l - C l (g) ⟶ C (s) + 2 H (g) + 2 C l (g)

Bond energy for C-H bond & C-Cl bond are 415KJ and 326KJ respectively.

Q. Use the bond energy data and calculate the enthalpy change for the above given reaction.
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The average bond energies of

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

Calculate the enthalpy ,

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$C = C$	$612$
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