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  • 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.

12.32.    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.

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best_answer

Given,
Percentage of carbon = 69%
% of Hydrogen = 4.8%, and 
% of Oxygen  =  26.2 %

So, 0.2 g of OC have (0.2\times 0.69)g of Carbon = 0.138g 
we know that,
molecular weight of  CO_{2} = 44 g
12 g of C is present in 44 g of CO_{2}

Therefore, 0.138 g of C present in 0.138\times \frac{44}{12} = 0.506 g of CO_{2}

Hence, from 0.2 g of OC 0.506 g of CO_{2} will be produced.

Similarly,
100 g  of OC contains 4.8 g of H
So, 0.2 g of OC contains (0.2\times 0.048) = 0.0096 g of H
We know the mol. wt. of water = 18 g

Therefore 0.0096 g of H will present in \frac{18\times 0.0096}{2} = 0.0864 g of water

Hence 0.2 gram of OC will produce 0.0864 g of water on complete combustion of

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