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Properties of Oxygen

The dissociat...

Question

The dissociation energy of $C H_{4}$ and $C_{2} H_{6}$ are respectively $360$ and $620 k c a l / m o l$ . The bond energy of $C - C$ bond is:

260 k c a l / m o l

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180 k c a l / m o l

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130 k c a l / m o l

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80 k c a l / m o l

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Solution

The correct option is B $80 k c a l / m o l$
The given that

Bond dissociation enthalpy of $C H_{4} = 360$ is the energy required to break $4 C - H$ bonds in it.

Thus dissociation enthalpy of $1 C - H$

$\frac{B o n d d i s s s o c i a t i o n e n t h a l p y o f C H_{4}}{4} = \frac{360}{4} = 90 k c a l / m o l .$

Bond dissociation enthalpy of $C_{2} H_{6} = 620$ is the energy required to break $6 C - H$ bonds in it.

$1 C - H$ bonds.

Thus, Bond dissociation enthalpy for $C - C$ = Bond dissociation enthalpy for $C_{2} H_{6} - 6$ (Bond dissociation enthalpy for $1 C - H)$

$\Rightarrow 620 - 6 (90) = 620 - 540$

$\Rightarrow 80 k c a l / m o l .$
This is the required solution.

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Similar questions

Q. Bond dissociation energy of

C H_{4} is 360 k J m o l^{- 1}

and

C_{2} H_{6} is 620 k J m o l^{- 1}

. Then bond dissociation energy of

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The enthalpy of atomisation of $C H_{4}$ and $C_{2} H_{6}$ are 360 and 620 k cal $m o l^{- 1}$ respectively. The C - C bond energy is expected to be ?

Q. The dissociation energy of

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Q. If the dissociation energy of

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The dissociation energy of CH4 and C2H6 are respectively 360 and 620 kcal/mol. The bond energy of C−C bond is:

The dissociation energy of $C H_{4}$ and $C_{2} H_{6}$ are respectively $360$ and $620 k c a l / m o l$ . The bond energy of $C - C$ bond is: