Question

0.2475 of an organic compound on combustion gave 0.4950 of CO2 and 0.2025 of H2O calculate the percentage of oxygen in the compound. ​

Answer 1

Explanation:

Compound → CO

2

+H

2

O

0.2475g 0.4950g 0.2025g

Mass of C in 0.2475g of compound = mass of C in 0.495g of CO

2

=

44

12

×0.495g

∴ % of C =

0.2475

12/44×0.495

×100 =54.54 %

Again mass of H in 0.2475g of Compound = mass of H in 0.2025g of H

2

S=

18

2

×0.2025g

∴ % of H =

0.2475

(2/18)×0.2025

×100 = 9.0 %

∴ % of oxygen =100−(%C +%H)= 100−( 54.54+9.2)=36.46%