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What is the $\Delta H$ of the reaction
The average bond energies of $\mathrm{C}-\mathrm{Cl}$ bond and $\mathrm{C}-\mathrm{H}$ bond are 416 kJ and $325 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.
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The average bond energies of $\mathrm{C}-\mathrm{Cl}$ bond and $\mathrm{C}-\mathrm{H}$ bond are 416 kJ and $325 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.
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Verified Answer
The correct answer is:
1482 kJ
In the reaction, two moles of $\mathrm{C}-\mathrm{H}$ bonds and two moles of $\mathrm{C}-\mathrm{Cl}$ bonds are broken.
Hence, energy absorbed
$\begin{aligned}
& =2 \times 416+2 \times 325 \\
& =1482 \mathrm{~kJ}
\end{aligned}$
Hence, energy absorbed
$\begin{aligned}
& =2 \times 416+2 \times 325 \\
& =1482 \mathrm{~kJ}
\end{aligned}$
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