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Heat of Formation

What is the ...

Question

What is the $Δ H$ of the reaction ?
The average bond energies of $C - C l$ bond and $C - H$ bond are $416 k J$ and $325 k J {m o l}^{- 1}$ respectively.

A

1482 k J

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B

1482 J

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C

1492 k J

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D

1492 J

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Solution

The correct option is B $1482 k J$
In the compound $C H_{2} {C l}_{2}$ , hter are 2 $C - C l$ and 2 $C - H$ bonds.

So total energy to dissociate
$C H_{2} {C l}_{2} ⟶ C + 2 H + 2 C l$
is $(2 * 416) + (2 * 325) = 1482 K J$

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Similar questions

Q. Calculate the

Δ H

of the reaction given (figure).
Bond energy for

C - H

C - C l

415 k J

326 k J

Q. Calculate the bond energy of

C l - C l

bond from the following data:

C H_{4 (g)} + C l_{(g)} \to C H_{3} C l_{(g)} + H C l_{(g)}; Δ H = - 100.3 k J

. Also the bond enthalpies of

C - H, C - C l, H - C l

413, 326

431

k J m o l^{- 1}

Q. If enthalpy of a reaction is

1482 k J / m o l

and bond dissociation enthalpy of

(C - H)

415 k J / m o l

than bond dissociation enthalpy of

(C - C l)

C H_{2} C l_{2 (g)} \to C_{(g)} + 2 H_{(g)} + 2 C l_{(g)}

Q. Calculate the

△

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.
The bond energies of

C - H

C - C l

413

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

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