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 compound is subjected to complete combustion.

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

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 compound is subjected to complete combustion.
Answer» Solution :Step I : Calculation of mass of `CO_(2)` produced Mass of compound `=0.20 G` Percentage of carbon `= 69%` Percentage of carbon `=12/44 xx ("Mass of carbon DIOXIDE formed")/("Mass of compound")XX100` `69=12/44xx("Mass of carbon dioxide formed")/((0.20 g))xx100` `:.` Mass of `CO_(2)` formed `=(69xx44xx(0.20 g))/(12xx100)=0.506 g` Step II. Calculation of mass of `H_(2)O` produced Mass of compound `=0.20 g` Percentage of hydrogen `= 4.8 %` Percentage of hydrogen `=2/18xx("Mass of water formed")/("Mass of compound")xx100` `4.8=2/10xx("Mass of water formed")/((0.20 g))xx100` `:.` Mass of `H_(2)O` formed `=(4.8xx18xx(0.20 g))/(2xx100)=0.0864 g`.