# Problem: Upon combustion, a 0.8009 g sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6003 g CO2 and 0.6551 g H2O. Find the empirical formula of the compound.

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###### FREE Expert Solution

Recall that in combustion analysis, a compound reacts with excess O2 to form products.

For a compound composed of C, H, and O, the reaction looks like this:

CxHyOz + O2 (excess)  x CO2y H2O

Calculate the mass of C and H.

Mass C:

molar mass of CO2 = 44.01 g/mol

There is 1 mole of C in 1 mole of CO2. Finding the mass of C:

mass of C = 0.4367 g C

Mass H:

molar mass of H2O = 18.02 g/mol

There are 2 moles of H in 1 mole of H2O. Finding the moles of H:

mass of H = 0.0734 g H

Calculate the mass of O:

We have 0.8009 g of the sample compound. Subtracting the masses of C and H from this will give us the mass of O:

mass of O = 0.8009 g – (0.4367 g C + 0.0734 g H) = 0.2908 g O

Calculate the moles of each element and determine the lowest whole number ratio.

moles of C = 0.0363 mol C

###### Problem Details

Upon combustion, a 0.8009 g sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6003 g CO2 and 0.6551 g H2O. Find the empirical formula of the compound.