Question

0.2033 g of an organic compound on combustion gives 0.3780 g of Co2 and 0.1238 gram H2O in separate experiment 0.1877 gram of the compound on analysis by Dumas method produced 31.7 ml of Nitrogen collected over Water at 14 degree Celsius and 758 mm pressure determine the percentage composition of the compound​

Answer 1

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

Explanation:

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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The percentage

The percentagecomposition of carbon

The percentagecomposition of carbonis 50.69 % and that of

The percentagecomposition of carbonis 50.69 % and that ofhydrogen is 6.9 %.