In the presence of oxygen an unknown hydrocarbon is burned in order to determine its empirical formula. Another sample of the hydrocarbon is subjected to colligative property tests in order to determine its molecular mass.
1. Determine the empirical formula of the hydrocarbon, if upon combustion at
STP, 9.01 grams of liquid H2O and 11.2 liters of CO2 gas are formed.
2. Calculate the mass of the oxygen gas that is used.
3. The hydrocarbon dissolves readily in CCl4. A solution prepared by missing the135 grams of CCl4 and 4.36grams of the hydrocarbon has the boiling point of 78.7 C. The molal boiling-point elevation constant of CCl4 is 5.02 C /molal, and its normal boiling point is 76.8 C. Determine the molecular weight of the hydrocarbon.
3. Calculate the molecular formula of the hydrocarbon.
a. Discuss how could you test if the tincture really disinfects drinking water? What experiment would you do?
b. Deter mine the purpose of alcohol (ethanol) in the process of making the iodine tincture?