Q48 / 150 · MHT CET 2024 (03 May Shift 2) · Chemistry
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 ?
- Correct answerA$416 \mathrm{~kJ} \mathrm{~mol}^{-1}$
- B$\quad-416 \mathrm{~kJ} \mathrm{~mol}^{-1}$
- C$832.5 \mathrm{~kJ} \mathrm{~mol}^{-1}$
- D$\quad-832.5 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Solution
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 $\begin{aligned} \mathrm{fCH}_4 & =\frac{-(-1665 \mathrm{~kJ})}{4} \\ & =416.25 \mathrm{~kJ} \end{aligned}$
Hence, the correct answer is option: 'A'.