An organic compound contains 69% carbon and 4.8% hydrogen, the remainder being oxygen. Calculate the masses of carbon dioxide and water produced when 0.20g of this substance is subjected to complete combustion

Explanation

Calculation of mass of water % `H= (2)/(18) xx (m_(1) xx 100)/(m)`
where % H= 4.8, mass of compound m= 0.2 gm, mass of `H_(2)O= m_(1)gm`
`therefore m_(1)= (% H xx 18 xx m)/(100 xx 2) = (4.8 xx 18 xx 0.2)/(100 xx 2)`
`=0.0864 gm H_(2)O`
Calculation of mass of `CO_(2)`
% `C = (12)/(44) xx (m_(2) xx 100)/(m)` where `m_(2)`= mass of `CO_(2)` %C= 69
`:. 69 = (12)/(44) xx (m_(2) xx 100)/(0.2)` m= mass of compound = 0.2gm
`therefore m_(2)= (69 xx 0.2 xx 44)/(100 xx 12)= 0.506gm`