JEE MAIN - Chemistry (2024 - 31st January Morning Shift - No. 27)
Number of moles of methane required to produce $$22 \mathrm{~g} \mathrm{~CO}_{2(\mathrm{~g})}$$ after combustion is $$\mathrm{x} \times 10^{-2}$$ moles. The value of $$\mathrm{x}$$ is _________.
Answer
50
Explanation
$$\mathrm{CH}_{4(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\ell)}$$
$$\mathrm{n}_{\mathrm{CO}_2}=\frac{22}{44}=0.5 \text { moles }$$
So moles of $$\mathrm{CH}_4$$ required $$=0.5$$ moles i.e. $$50 \times 10^{-2} \mathrm{~mole}$$
$$\mathrm{x}=50$$
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