Question

0.2033 g of an organic compound on combustion gave 0.3780 of carbon dioxide and 0.1288 h20 .In a separate experiment 0.1877 g of the compound on analysis by Dumas method produced 31.7 ml of nitrogen collected over waterway 14 C and 758 mm pressure. Determine the percentage composition of the compound. (aqueous tension of water at 14 c =12mm pressure) C=50.7,H=7.04 N =19.7 and 0=22.55​

Answer 1

The percentage composition of carbon is 50.69 % and that of hydrogen is 6.9 %.

Explanation:

0.2033 g of an organic compound on combustion gave 0.3780 of carbon dioxide and 0.1288 H2O. Determine the percentage composition of carbon and hydrogen.

Solution:

We are given that:

Wt of CO2 = 0.3780 g

Wt of H2O = 0.1288 g

wt of Organic compound = 0.2033 g

% of C = 12/44 x Wt. of CO2 / total wt of compound x 100

% of C = 12/44 x 0.3780 / 0.2033 x 100

% of C = 0.2727 x 1.859 x 100

% of C = 50.69 %

% of H = 2 / 18 x 0.1288 / 0.2033  x 100

% of H = 0.11 x 0.6335 x 100

% of H = 6.9 %

Thus the percentage composition of carbon is 50.69 % and that of hydrogen is 6.9 %.

Answer 2

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