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 `= 69%`
Amount of carbon in `0.20` g of compound `= 0.2 xx (69)/(100)=0.138` g
Percentage of hydrogen `= 4.8%`
Amount of hydrogen in `0.20 g ` of compound `= (0.2 xx 4.8)/(100)= 0.0096` g
Now `C -= CO_2`
`12` g of carbon on combustion give `CO_2 = 44` g
`0.138` g of carbon on combustion give `CO_2 = (44)/(12) xx 0.138= 0.506` g
`2H = H_2 O`
`2` g of hydrogen on combustion give water `= 18` g
`0.0096` g of hydrogen on combustion give water `= (18)/(2) xx 0.0096= 0.0864` g