Enthalpy of polymerization of ethylene. as represented by the reaction
$_{n} {CH}_{2} = {CH}_{2} ⟶ {(- {CH}_{2} - {CH}_{2} -)}_{n} is - 100 kJ$ Per mole of ethylene. Given bond enthalpy of $C = C$ bond is $600 k J m o l^{- 1}$ , enthalpy of $C - C$ bond (in $kJ$ ) will be :

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700

indeterminate

350

116. 7

answer is B.

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Detailed Solution

Every mole of ethylene contains two single bonds when it is polymerized completely.

$Δ H_{polymerisation} = Δ H_{({CH}_{2} = {CH}_{2})} - 2 {ΔH}_{({CH}_{2} - {CH}_{2})}$

$2 Δ H_{({CH}_{2} - {CH}_{2})} = 600 - (- 100) = 700 k J m o l^{- 1}$

$2 Δ H_{(C H_{2} - C H_{2})} = \frac{700}{2} = 350 k J {mol}^{- 1}$

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