NCERT Class XI Chemistry Organic Chemistry Some basic principles and Techniques Solutions

Question : 32

Total: 40

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 g of this substance is subjected to complete combustion.

Solution:

Given : % of carbon = 69; % of hydrogen = 4.8
% of oxygen = 100 – (69 + 4.8) = 26.2
Mass of compound = 0.2 g
100 g of compound contains 69 g of C
0.2 g of compound contains

69×0.2

100

= 0.138 g of C
Also, 12 g of C produces 44 g of CO2
∴ 0.138 g of C will give =

44×0.138

= 0.506 g of CO2
100 g of compound contains 4.8 g of H
∴ 0.2 g of compound contains

4.8×0.2

100

= 0.0096 g of H
Also, 2 g of H produces 18 g of H2O
∴ 0.0096 g of H produces

18×0.0096

g = 0.0864 g of H2O
Thus, mass of CO2 produced = 0.506 g and mass of H2O produced = 0.0864 g

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