On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of $\mathrm{CO}_2$ and 0.567 g of $\mathrm{H}_2 \mathrm{O}$. The empirical formula mass of compound $(\mathrm{X})$ is ________ g.
(Given molar mass in $\mathrm{g} \mathrm{mol}^{-1} \mathrm{C}: 12, \mathrm{H}: 1, \mathrm{O}: 16$)

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Aicharya · Accepted Answer

Moles of ' C ' $=\mathrm{n}_{\mathrm{CO}_2}=\frac{1.46}{44}=0.033$ Moles of ' C ' $=\mathrm{W}_{\mathrm{C}}=0.033 \times 12$ Moles of 'H' $=2 \times \mathrm{n}_{\mathrm{H}_2 \mathrm{O}}=2 \times \frac{0.567}{18}=0.063$ Mass of ' H ' $=0.0063$ Mass of Oxygen $(\mathrm{O})=1-\left(\mathrm{W}_{\mathrm{c}}+\mathrm{W}_{\mathrm{H}}\right)$ $=1-(0.033 \times 12+0.063 \times 1)=0.541 \mathrm{gm}$ Moles of ' O ' $=\frac{0.541}{16}=0.033$ Empirical formula $=\mathrm{CH}_2 \mathrm{O}$ Empirical formula mass $=30$.

On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of \(\mathrm{CO}_2\) and 0.567 g of…

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