Question

The complete combustion of $0.492g$ of an organic compound containing ' $C$ ', ' $H$ ' and ' $O$ ' gives $0.793g$ of $C{O}_2$ and $0.442g$ of $H_{2}O$. The percentage of oxygen composition in the organic compound is __(nearest integer)

Answer 1

Answer: 46

Mole of $C{O}_2=$ Moles of $C=\frac{0.793}{44}$
Weight of ' $C$ ' $=\frac{0.793}{44}\times 12=0.216gm$
Moles of ' $H^{\prime }=\frac{0.442}{18}\times 2$
Weight of ' $H^{\prime }=\frac{0.442}{18}\times 2\times 1=0.049gm$
$\therefore$ Weight of ' $O$ ' $=0.492-0.216-0.049=0.227gm$
$\%$ of ' ${}^{\prime }{}^{\prime }=\frac{0.227}{0.492}\times 100=46.13\%$