# Problem: A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces 33.5 mg CO2 and 41.1 mg H2O. What is the empirical formula of the compound?

###### FREE Expert Solution
• Determine the empirical formula by calculating the moles of C, H and N present in the compound. This can be calculated using the provided mass of CO2 and H2O
• We can directly assume that all the C in the compound are converted to CO2 while the Hs go to H2O
• Establish a relationship using stoichiometry to get the moles of C and O.
• Mass of N (eventually moles) can be calculated once we already have the mass of C and H
• 1 mole CO2 contains 1 mole C while H2O contains 2 moles of H. Calculation of mass and mole of C will appear as:

molar mass of CO2

C - 12.01 (1) = 12.01

O - 16 (2) = 32

12.01 + 32 = 44.01 g/mol

molar mass of H2O:

H - 1.01 (2) = 2.02

O - 16 (1) = 16

16 + 2.02 = 18.02 g/mol ###### Problem Details

A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces 33.5 mg CO2 and 41.1 mg H2O. What is the empirical formula of the compound?