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An organic compound contains \(69 \%\) carbon and 4. \(8 \%\) hydrogen, the remainder being oxygen. Calculate the masses of carbon dioxide and water produced when \(0.20 \mathrm{~g}\) of this substance is subjected to complete combustion.
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We know that \(\% \mathrm{C}=12 / 44 \times\left(\right.\) Mass of \(\mathrm{CO}_2\) formed \() /(\) Mass or substance taken \() \times 100\)
Substituting the values of \(\%\) of \(\mathrm{C}\) and mass of the substance taken, we have,
\(69=\frac{12}{44} \times \frac{\text { mass of } \mathrm{CO}_2 \text { formed } \times 100}{\text { mass of substance taken }}\)
or Mass of \(\mathrm{CO}_2\) formed \(=\frac{69 \times 44 \times 0.2}{12 \times 100}=0.506 \mathrm{~g}\)
Similarly, \(\% \mathrm{H}=2 / 18 \times\left(\right.\) Mass of \(\mathrm{H}_2 \mathrm{O}\) formed \() /\) mass of substance taken \(\times 100\)
Substituting the values of \(\% \mathrm{H}\) and the mass of substance taken, we have,
\(4.8=\frac{2 \times \text { mass of water formed }}{18 \times 0.2} \times 100\) or mass of water formed \(=\frac{4.8 \times 18 \times 0.2}{2 \times 100}=0.0864 \mathrm{~g}\)
Substituting the values of \(\%\) of \(\mathrm{C}\) and mass of the substance taken, we have,
\(69=\frac{12}{44} \times \frac{\text { mass of } \mathrm{CO}_2 \text { formed } \times 100}{\text { mass of substance taken }}\)
or Mass of \(\mathrm{CO}_2\) formed \(=\frac{69 \times 44 \times 0.2}{12 \times 100}=0.506 \mathrm{~g}\)
Similarly, \(\% \mathrm{H}=2 / 18 \times\left(\right.\) Mass of \(\mathrm{H}_2 \mathrm{O}\) formed \() /\) mass of substance taken \(\times 100\)
Substituting the values of \(\% \mathrm{H}\) and the mass of substance taken, we have,
\(4.8=\frac{2 \times \text { mass of water formed }}{18 \times 0.2} \times 100\) or mass of water formed \(=\frac{4.8 \times 18 \times 0.2}{2 \times 100}=0.0864 \mathrm{~g}\)
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