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.

Explanation

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`.