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

Amount of C in 0.2g of compound `=0.2xx(69)/(100)=0.138g`
Now, `C=CO_(2)`
12 g of carbon given 44g `CO_(2)` on combustion
`therefore 0.138g` of carbon give `(44)/(12)xx0.138g=0.506 g`
Amount of H in 0.2g of compound =`0.2xx(4.8)/(100)=0.0096g`
Now, 2H=`H_(2)O`
2g of hydrogen gives 18g water on combustion
`therefore 0.0096` g of hydrogen given `(18)/(2)xx0.0096g=0.0864g`