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 gm of this substance is subjected to complete combustion.

Explanation

Percentage of carbon in organic compound = 69%
That is, 100 g of organic compound contains 69 g of carbon.
`therefore` 0.2 g of organic compound will contain `=(69xx0.2)/100=0.138g` of C
Molecular mass of carbon dioxide, `CO_(2)` = 44 g
That is, 12 g of carbon is contained in 44 g of `CO_(2)`.
Therefore, 0.138 g of carbon will be contained in `(44xx0.138)/12=0.506`g of `CO_(2)`
Thus, 0.506 g of `CO_(2)` will be produced on complete combustion of 0.2 g of organic compound.
Percentage of hydrogen in organic compound is 4.8.
i.e., 100 g of organic compound contains 4.8 g of hydrogen.
Therefore, 0.2 g of organic compound will contain `(4.8xx0.2)/100=0.0096`g of H
It is known that molecular mass of water `(H_(2)O)` is 18 g.
Thus, 2 g of hydrogen is contained in 18 g of water.
`therefore` 0.0096 g of hydrogen will be contained in `(18xx0.0096)/2=0.0864`g of water
Thus, 0.0864 g of water will be produced on complete combustion of 0.2 g of the organic compound.