5.A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 72.0 seconds for 1.00 L of the gas to effuse. Under identical experimental conditions it required 28.0 seconds for 1.00 L of oxygen gas to effuse. Calculate the molar mass of the unknown gas. Remember that the faster the rate of effusion, the shorter the time required for effusion, the rate is inversely proportional.

5.A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 72.0 seconds for 1.00 L of the gas to effuse. Under identical experimental conditions it required 28.0 seconds for 1.00 L of oxygen gas to effuse. Calculate the molar mass of the unknown gas. Remember that the faster the rate of effusion, the shorter the time required for effusion, the rate is inversely proportional.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A sample of an unknown gas effuses in 11.8 min. An equal volume of H2 in the same apparatus at the same temperature and pressure effuses in 2.16 min. What is the molar mass of the unknown gas?
The rate of effusion of an unknown gas was measured and found to be 11.9 mL/min. Under identical conditions, the rate of effusion of pure oxygen (O,) gas is 14 mL/min. Based on this information, the identity of the unknown gas could be: O NO CO, F2
Effusion is the process where a gas flows through a small hole in a container. Graham’s Law of Effusion says that the rate of effusion of a gas from a particular hole is inversely proportional to the square root of the MW of the gas (at constant temperature and pressure). Describe why normal balloons filled with He tend to go flat faster than the same balloons filled with air.
The rate of a particular gas was measured and found to be 24.0 mL/min. Under the same conditions, the rate of effusion of pure methane (CH4) gas is 47.8 mL/min. What is the molar mass of the unknown gas?
At a particular pressure and temperature, nitrogen gas effuses at the rate of 79 mL/s. Using the same apparatus at the same temperature and pressure, at what rate will sulfur dioxide effuse?
A 1.56 mol sample of O2 gas is confined in a 37.6 liter container at 20.9 °C. If 1.56 mol of H2 gas is added and the volume and temperature of the system are held constant, explain in at least one sentence what will happen to... a. The average molecular speed of the system. In your answer, you should indicate whether the average molecular speed will increase, decrease or remain the same, and also indicate your reasoning why. b. The average kinetic energy of the system. In your answer, you should indicate whether the average kinetic energy will increase, decrease or remain the same, and also indicate your reasoning why.
Constants | Periodic Table A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure conditions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 29 s for 1.0 L of O2 gas to effuse. ▾ Part A Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) Express your answer in grams per mol to two significant figures. M = Ο ΑΣΦ Submit Request Answer 3+ < Return to Assignment Provide Feedback a % ? g/mol MacBook Pro 曲 C
An unknown gas effuses at a rate that is .462 times that of nitrogen gas (at the same temperature). Calculate the molar mass of the unknown gas in mol/L.
A sample of unknown gas and N2 are allowed to effuse from the same apparatus. The unknown gas effuses at the rate of 5.45 ml/s, whereas the N2 effuses at the rate of 9.55 ml/s. What is the molar mass of the unknown gas?
A student was assigned the task of determining the molar mass of an unknown gas. The student measured the mass of a sealed 843 mL rigid flask that contained dry air. The student then flushed the flask with the unknown gas, resealed it, and measured the mass again. Both the air and the unknown gas were at 23.0°C and 750. torr. The data for the experiment are shown in the table below. Volume of sealed flask 843 mL Mass of sealed flask and dry air 157.70 g Mass of sealed flask and unknown gas 157.40 g Calculate the mass, in grams, of the dry air that was in the sealed flask. (The density of dry air is 1.18 g L−1 at 23.0°C and 750. torr.) g air Calculate the moles of air that were in the sealed flask. moles air Calculate the mass, in grams, of the sealed flask itself (i.e., if it had no air in it). g Calculate the mass, in grams, of the unknown gas that was added to the sealed flask. g unknown gas Using the information above, calculate the value of the molar mass…
An unknown gas effuses at a rate of 2.00 times the rate of Cl₂. What is the molar mass of the unknown gas?
Under conditions in which the density of carbon dioxide is 1.96 g/L and that of nitrogen is1.25 g/L, which gas will effuse more rapidly? What will be the ratio of the rates of effusion ofnitrogen to carbon dioxide?