Q19 / 150 · MHT CET 2023 (12 May Shift 1) · Chemistry
Calculate amount of methane formed by liberation of $149.6 \mathrm{~kJ}$ of heat using following equation.
$$
\mathrm{C}_{(\mathrm{s})}+2 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{CH}_{4(\mathrm{~g})} \quad \Delta \mathrm{H}=-74.8 \mathrm{~kJ} / \mathrm{mol}
$$
- A$16 \mathrm{~g}$
- B$24 \mathrm{~g}$
- Correct answerC$32 \mathrm{~g}$
- D$48 \mathrm{~g}$
Solution
According to the given reaction, $74.8 \mathrm{~kJ}$ of heat is evolved when 1 mol of methane is formed.
$$
\begin{aligned}
& 74.8 \mathrm{~kJ} \equiv 1 \mathrm{~mol} \mathrm{CH}_4=16 \mathrm{~g} \mathrm{CH}_4 \\
& 149.6 \mathrm{~kJ} \equiv x \mathrm{~g} \mathrm{CH}_4 \\
& x=\frac{149.6 \times 16}{74.8}=32 \mathrm{~g}
\end{aligned}
$$
Hence, the correct answer is option: 'C'.