What will be - H for the reaction- CH2Cl2 - C - 2H - 2Cl-B-E- of C - H and C - Cl bonds are 416 kJ mol-1 and 325 kJ mol-1 respectively

The correct option is D 1482 kJ Δ H=∑BE_R ∑BE_P #160; #160; #160; #160; #160; =2× BE(C H)+2× BE(C Cl) #160; #160; #160; ...

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Standard XII

Physics

Calorimetry

What will be ...

Question

What will be $Δ H$ for the reaction,
$C H_{2} C l_{2} \to C + 2 H + 2 C l$ ?
(B.E. of C - H and C - Cl bonds are 416 kJ $m o l^{- 1}$ and 325 kJ $m o l^{- 1}$ respectively)

832 kJ

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1482 kJ

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650 kJ

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1855 kJ

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Solution

The correct option is D 1482 kJ
$Δ H = \sum B E_{R} - \sum B E_{P}$
$= 2 \times B E (C - H) + 2 \times B E (C - C l)$
$= 2 \times 416 + 2 \times 325$
$= 1482 k J$

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Similar questions

Q. 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.

Q. Calculate

△ H_{r}^{o}

for the reaction

C H_{2} C l_{2} (g) \to C (g) + 2 H (g) + 2 C l (g) .

The average bond enthalpies of C - H and C - Cl bonds are

414 k J m o l^{- 1}

and

330 k J m o l^{- 1} .

Q. Calculate

△ H_{r}^{o}

for the reaction

C H_{2} C l_{2} (g) \to C (g) + 2 H (g) + 2 C l (g) .

The average bond enthalpies of C - H and C - Cl bonds are

414 k J m o l^{- 1}

and

330 k J m o l^{- 1} .

Given that bond energies of
$H - H$ and $C l - C l$ are $430 k J m o l^{- 1}$ and $240 k J m o l^{- 1}$ respectively and $Δ_{f} H$ for $H C l$ is -90 kJ $m o l^{- 1} .$ The bond enthalpy of $H C l$ is:

Q. Bond energies of some bonds are given below:
Cl-Cl = 242.8 kJ

m o l^{- 1}

, H-Cl = 431.8 kJ

m o l^{- 1}

,
O-H = 464 kJ

m o l^{- 1}

, O=O = 442 kJ

m o l^{- 1}

Using the B.E.s given, calculate

Δ H

for the given reaction:

2 C l_{2} + 2 H_{2} O \to 4 H C l + O_{2}

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What will be ΔH for the reaction,CH2Cl2→C+2H+2Cl?(B.E. of C - H and C - Cl bonds are 416 kJ mol−1 and 325 kJmol−1 respectively)

The correct option is D 1482 kJΔH=∑BER−∑BEP =2×BE(C−H)+2×BE(C−Cl) =2×416+2×325 =1482 kJ

What will be $Δ H$ for the reaction,
$C H_{2} C l_{2} \to C + 2 H + 2 C l$ ?
(B.E. of C - H and C - Cl bonds are 416 kJ $m o l^{- 1}$ and 325 kJ $m o l^{- 1}$ respectively)

The correct option is D 1482 kJ
$Δ H = \sum B E_{R} - \sum B E_{P}$
$= 2 \times B E (C - H) + 2 \times B E (C - C l)$
$= 2 \times 416 + 2 \times 325$
$= 1482 k J$