Complete combustion of 1.80 g of an oxygen containing compound ( C x H y O 2) gave 2.64 g of CO 2 and 1.08 g of H 2 O. The percentage of oxygen in the organic compound is:

Question

Complete combustion of 1.80 g of an oxygen containing compound ( C x H y O 2) gave 2.64 g of CO 2 and 1.08 g of H 2 O. The percentage of oxygen in the organic compound is: (A) 51.63 (B) 63.53 (C) 53.33 (D) 50.33

Tardigrade Admin · Accepted Answer

n c = n co 2=(2.64/44)=0.06 n H =2 × n H 2 O =(1.08/18) × 2=0.12 m 0=1.80-12 × (2.64/44)-(1.08/18) × 2 =1.80-0.72-0.12=0.96 gm % 0=(0.96/1.80) × 100=53.33 %

Q. Complete combustion of $1.80 g$ of an oxygen containing compound $(C_{x} H_{y} O_{2})$ gave $2.64 g$ of $C O_{2}$ and $1.08 g$ of $H_{2} O$ . The percentage of oxygen in the organic compound is:

51.63

63.53

53.33

50.33

$n_{c} = n_{c o_{2}} = \frac{2.64}{44} = 0.06$

$n_{H} = 2 \times n_{H_{2} O} = \frac{1.08}{18} \times 2 = 0.12$

$m_{0} = 1.80 - 12 \times \frac{2.64}{44} - \frac{1.08}{18} \times 2$

$= 1.80 - 0.72 - 0.12 = 0.96 g m$

$%0 = \frac{0.96}{1.80} \times 100 = 53.33%$

Q. Complete combustion of 1.80g of an oxygen containing compound (Cx​Hy​O2​) gave 2.64g of CO2​ and 1.08g of H2​O. The percentage of oxygen in the organic compound is: