Question

calculate the percentage of c in organic compund gave on combustion 0.4950 g of carbon dioxide and 0.2475 g of water

Answer 1

(i) Given data:

Mass of organic compound = 0.2475 g

Mass of carbon dioxide produced = 0.4950 g

Mass of water produced = 0.2025 g

Let us find the % of C and H present in the compound

% of Carbon= (12/44 )X (mass of CO2/ Mass of compound taken) X 100

= (12/44 )X (44/0.2475) X 100 = 54.54

% of H =( 2/18) X (mass of H2O/Mass of compound taken) X 100

= (2/18)X (18/0.2475) X100 = 9.09(ii)  If the compound contains both nitrogen and sulphur during lassaigne's test they combine with sodium metal to form Sodium thiocyanate. This compound on reaction with ferric chloride form ferric thiocyanate (FeCNS)3 which is blood red in color.

Answer 2

hi friends...
here is your ans....

Mass of organic compound = 0.2475 g

Mass of carbon dioxide produced = 0.4950 g

Mass of water produced = 0.2025 g

Let us find the % of C and H present in the compound

% of Carbon= (12/44 )X (mass of CO2/ Mass of compound taken) X 100

= (12/44 )X (44/0.2475) X 100 = 54.54

% of H =( 2/18) X (mass of H2O/Mass of compound taken) X 100

= (2/18)X (18/0.2475) X100 = 9.09 (ii)  If the compound contains both nitrogen and sulphur during lassaigne's test they combine with sodium metal to form Sodium thiocyanate. This compound on reaction with ferric chloride form ferric thiocyanate (FeCNS)3 which is blood red in color