7. Gases

Effusion

7. Gases

Effusion

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Chemistry of Gases (37 of 40) Effusion of Gases: Basics

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Chemistry of Gases (37 of 40) Effusion of Gases: Basics

Gas Diffusion, Effusion, Graham's Law Practice Problems & Examples Calculation

Chemistry 7.7 Diffusion Effusion and Graham's Law

Effusion and Diffusion of Gases

Difference between Diffusion and Effusion Class 11 Chemistry |Real Life Examples | Gaseous State

Graham's Law of Effusion

The Organic Chemistry Tutor

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Practice Problem: Graham's Law of Effusion

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Practice Problem: Graham's Law of Effusion

Professor Dave Explains

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Multiple Choice

If H₂has an effusion rate that is 3.72 times faster than a gas, what is the identity of the unknown gas?

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Multiple Choice

How many times faster will H₂ gas pass through a pinhole into an area of vacuum than O₂ gas?

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Multiple Choice

It takes 6.3 minutes for 2.3 L argon to effuse through a semipermeable membrane. How long would it take for 2.3 L of chlorine gas to effuse under similar conditions?

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Multiple Choice

Determine the identity of an unknown gas that effuses at a rate 1.48 times as fast as chlorine gas.

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Textbook Question

The apparatus shown here has two gas-filled containers and one empty container, all attached to a hollow horizontal tube. When the valves are opened and the gases are allowed to mix at constant temperature, what is the distribution of atoms in each container?

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Textbook Question

A thin glass tube 1 m long is filled with Ar gas at 101.3 kPa, and the ends are stoppered with cotton plugs as shown below. HCl gas is introduced at one end of the tube, and simultaneously NH3 gas is introduced at the other end. When the two gases diffuse through the cotton plugs down the tube and meet, a white ring appears due to the formation of NH4Cl1s2. At which location—a, b, or c—do you expect the ring to form?

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Textbook Question

An unknown gas is found to diffuse through a porous membrane 2.92 times more slowly than H2. What is the molecular weight of the gas? (a) 17.0 g/mol (b) 5.84 g/mol (c) 8.52 g/mol

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Textbook Question

Which one or more of the following statements are true? (a) O2 will effuse faster than Cl2. (b) Effusion and diffusion are different names for the same process. (c) Perfume molecules travel to your nose by the process of effusion. (d) The higher the density of a gas, the shorter the mean free path.

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Textbook Question

Calculate the root mean square velocity and kinetic energy of F2, Cl2, and Br2 at 298 K. Rank these three halogens with respect to their rate of effusion.

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Textbook Question

Hydrogen has two naturally occurring isotopes, 1H and 2H. Chlorine also has two naturally occurring isotopes, 35Cl and 37Cl. Thus, hydrogen chloride gas consists of four distinct types of molecules: 1H35Cl, 1H37Cl, 2H35Cl, and 2H37Cl. Place these four molecules in order of increasing rate of effusion.

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Textbook Question

We separate U-235 from U-238 by fluorinating a sample of uranium to form UF6 (which is a gas) and then taking advantage of the different rates of effusion and diffusion for compounds containing the two isotopes. Calculate the ratio of effusion rates for 238UF6 and 235UF6. The atomic mass of U-235 is 235.054 amu and that of U-238 is 238.051 amu.

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Textbook Question

Calculate the ratio of effusion rates for Ar and Kr.

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Textbook Question

Arsenic(III) sulfide sublimes readily, even below its melting point of 320 °C. The molecules of the vapor phase are found to effuse through a tiny hole at 0.52 times the rate of effusion of Xe atoms under the same conditions of temperature and pressure. What is the molecular formula of arsenic(III) sulfide in the gas phase?

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Textbook Question

A sample of neon effuses from a container in 76 seconds. The same amount of an unknown noble gas requires 155 seconds. Identify the second gas.

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Textbook Question

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 31 s for 1.0 L of O2 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 of 1.0 L; in other words, rate is the amount that diffuses over the time it takes to diffuse.)

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Textbook Question

A sample of N2O effuses from a container in 42 seconds. How long will it take the same amount of gaseous I2 to effuse from the same container under identical conditions?

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Textbook Question

What is the difference between effusion and diffusion?

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Textbook Question

Why does a helium-filled balloon lose pressure faster than an air-filled balloon?

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