6. In the molecular weight determination by the Dumas method, as illustrated below, several grams of an organic liquid were drawn into the bulb. The bulb was then immersed in a water bath at 87°C and kept there until all the liquid was vaporized and the air in the bulb was replaced by the vapor. The tip was then sealed shut and the bulb removed from the bath, cooled, dried and weighed at room temperature. The weight of the bulb filled with the vapor was 36.127 g the weight of the empty (evacuated) bulb was 35.427 g; the bulb's volume was 200.0 mL; room temperature was 250C; and the barometric pressure was 720 mm Hg. Calculate the molecular weight of the organic liquid.

6. In the molecular weight determination by the Dumas method, as illustrated below, several grams of an organic liquid were drawn into the bulb. The bulb was then immersed in a water bath at 87°C and kept there until all the liquid was vaporized and the air in the bulb was replaced by the vapor. The tip was then sealed shut and the bulb removed from the bath, cooled, dried and weighed at room temperature. The weight of the bulb filled with the vapor was 36.127 g the weight of the empty (evacuated) bulb was 35.427 g; the bulb's volume was 200.0 mL; room temperature was 250C; and the barometric pressure was 720 mm Hg. Calculate the molecular weight of the organic liquid.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.74QE: Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman...

See similar textbooks

Similar questions

Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
Describe how 500 mL of a 1.5 M solution of HCl prepared from 12.1 M HCl and pure solvent.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?