# 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.

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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