Combustion analysis of toluene, a compound containing carbon and hydrogen only, gives 5.86 mg carbon dioxide and 1.37 mg of water. What is its empirical formula?
Menthol is composed of carbon, hydrogen and oxygen. A 1.005 g sample is combusted, producing 0.2829 g carbon dioxide and 0.1159 g of water. If the molar mass of menthol is 156 g/mol, what are the empirical and molecular formulas of menthol?
Please provide detailed explanation.
1. Solve for the mass of carbon from the given the mass of carbon dioxide.
mass of CO2 = 5.86 mg = 0.00586 g
mass of C = 0.00586 g CO2 x (12 g C/44 g CO2)
mass of C = 1.598 x 10-3 g
Note: 1 mole CO2 contains 1 mole C, hence, the mass of C relative to the mass of CO2 is (12 g C/44 g CO2).
2. Solve for the mass of hydrogen from the given the mass of water.
mass of H2O = 1.37 mg = 0.00137 g
mass of H = 0.00137 g H2O x (2 g H/18 g H2O)
mass of H = 1.522 x 10-4 g
Note: 1 mole H2O contains 2 moles H, hence, the mass of H relative to the mass of H2O is (2 g H/18 g H2O).
3. Determine the empirical formula of the compound.
Mnemonics in finding the empirical formula:
*Mass to Mole*
*Divide by small*
*Multiply ’till whole*
Elements in the …
The expert examines a combustion analysis of toluene. The molar mass of menthol is analyzed.To continue with the answer check on mycoursewriter.com/
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