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 1. Calculation of mass of `CO_(2)` produced
Mass of compound = 0.20 g
Percentage of carbon = 69 g
`"Percentage of carbon"=(12)/(44)=("Mass of carbon dioxide formed")/("Mass of compound") xx 100`
`69= (12)/(44)=("Mass of carbon dioxide formed")/((0.20g)) xx 100`
`:. "Mass of" CO_(2) "formed" = (69 xx 44 xx (0.20g))/(12 xx 100)=0.506g`
Step II. Calculation of mass of `H_(2)O` produced
Mass of compound=0.20g
Percentage of hydrogen = 4.8%
`4.8 = (2)/(18) xx ("Massof water formed")/("Mass of compound") xx 100`
`:. "Mass of" H_(2)O "formed"=(4.8 xx 18 xx (0.20 g))/(2 xx 100)=0.0864 g`