11. Caproic acid, which is responsible for the foul odor of dirty socks, is composed of C, H, and O atoms. Combustion of a 0.225-g sample of this compound produces 0.512 g CO2 and 0.209 g H2O. (a) What is the empirical formula of caproic acid

C3H6O

Explanation:

Step 1:

Data obtained from the question include the following:

Mass of the compound = 0.225g

Mass of CO2 = 0.512g

Mass of H2O = 0.209g

Step 2:

Determination of the masses of carbon, hydrogen and oxygen present in the compound.

This is illustrated below:

For Carbon, C:

Molar mass of CO2 = 12 + (2x16) = 44g/mol

Mass of C in CO2 = 12/44 x 0.512 = 0.1396g

For Hydrogen, H:

Molar mass of H2O = (2x1) + 16 = 18g/mol

Mass of H in H2O = 2/18 x 0.209 = 0.0232g

For Oxygen, O:

Mass of O = 0.225 – (0.1396 + 0.0232)

Mass of O = 0.0622g

Step 3:

Determination of the empirical formula for caprioc acid.

This can be obtain as follow:

C = 0.1396g

H = 0.0232g

O = 0.0622g

Divide by their molar mass

C = 0.1396/12 = 0.0116

H = 0.0232/1 = 0.0232

O = 0.0622/16 = 0.0039

Divide by the smallest

C = 0.0116/0.0039 = 3

H = 0.0232/0.0039 = 6

O = 0.0039/0.0039 = 1

Therefore, the empirical formula for caprioc acid is C3H6O

the dependant variable is spilled water

the independent is the heat