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.

An organic compound contains 69% carbon and 4.8% hydrogen, the remaind

1.	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.
Answer» Solution :We know that, `%C = (12)/(44) xx ("Mass of " CO_(2) " formed")/("Mass of SUBSTANCE taken") xx 100` Substituting the values of % of C and mass of the substance taken, we have, `69 = (12)/(44) xx ("mass of " CO_(2) " formed")/(0.2g) xx 100` or Mass of `CO_(2)` formed `= (69 xx 44 xx 0.2)/(12 xx 100) = 0.506 g` Similarly, `%H = (2)/(18) xx ("Mass of" H_(2)O " formed")/("Mass of substance taken") xx 100` Substitutingthe values of % of H and mass of the substance taken, we have, `4.8 = (12)/(18) xx ("Mass of " H_(2)O " formed")/(0.2) xx 100` or Mass of `H_(2)O` formed `= (4.8 xx 18 xx 0.2)/(2 xx 100) = 0.0864 g`.