MHT CET · Chemistry · Thermodynamics (C)
Given that \(\mathrm{C}_{(\mathrm{g})}+4 \mathrm{H}_{(\mathrm{g})} \longrightarrow \mathrm{CH}_{4(\mathrm{~g})} \Delta \mathrm{H}^{\circ}=-1665 \mathrm{~kJ}\) What is bond energy per mole of \(\mathrm{C}-\mathrm{H}\) bond ?
- A \(416 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
- B \(-416 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
- C \(832.5 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
- D \(-832.5 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
Answer & Solution
Correct Answer
(A) \(416 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
Step-by-step Solution
Detailed explanation
In the given reaction, there are \(4 \mathrm{C}-\mathrm{H}\) bonds formed per mole of \(\mathrm{CH}_4\).
Bond energy per mole of
\(\begin{aligned}
\mathrm{fCH}_4 & =\frac{-(-1665 \mathrm{~kJ})}{4} \\
& =416.25 \mathrm{~kJ}
\end{aligned}\)
Bond energy per mole of
\(\begin{aligned}
\mathrm{fCH}_4 & =\frac{-(-1665 \mathrm{~kJ})}{4} \\
& =416.25 \mathrm{~kJ}
\end{aligned}\)
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