7. Gases

Effusion

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

Effusion Example 2

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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Effusion Example 1

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.

What is the molecular weight of a gas that diffuses through 
a porous membrane 1.86 times faster than Xe? What might 
the gas be?

Rank the following gases in order of their speed of diffusion 
through a membrane, and calculate the ratio of their 
diffusion rates: HCl, F2, Ar.

Chlorine occurs as a mixture of two isotopes, 35Cl and 
37Cl. What is the ratio of the diffusion rates of the three 
species 135Cl22, 35Cl37Cl, and 137Cl22?

Chemistry 7.7 Diffusion Effusion and Graham's Law

If H2&nbsp;has an effusion rate that is 3.72 times faster than a gas, what is the identity of the unknown gas?

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.)

Practice Problem: Graham's Law of Effusion

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

Effusion and Diffusion of Gases

 Using Graham&#8217;s law, the molar mass of the unknown gas is approximately 32 g/mol. 

 Correct, the molar mass based on the data is closest to that of molecular oxygen. 

The rate of effusion of a gas is inversely proportional to the square root of the molar mass of the gas. Graham&#8217;s law of effusion states: rateA/rateB = &#8730;(MB/MA).

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

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.

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.

What is the difference between effusion and diffusion?

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

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

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?

Graham's Law of Effusion

Calculate the ratio of effusion rates for Ar and Kr.

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

Which will diffuse through a membrane more rapidly, CO
or N2? Assume that the samples contain only the most
abundant isotopes of each element, 12C, 16O, and 14N.

In a given diffusion apparatus, 15.0 mL of HBr gas diffuses in
1.0 min. In the same apparatus and under the same conditions,
20.3 mL of an unknown gas diffuses in 1.0 min. The unknown
gas is a hydrocarbon. Find its molecular formula.

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.

Consider the following gases, all at STP: Ne, SF6, N2, CH4.
(f) Which one would effuse more rapidly than N2? 

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

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?

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?

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.

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? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/89d2024401d1a7ba-1664287427710.jpg" alt="" />

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Conquer Chemistry

1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Partial Pressure

Partial Pressure (PGas) is the pressure exerted by an individual gas within a container.

Velocity Distributions

Velocity Distributions represent probability distributions for a gas when examining their molar mass and temperature.

Mole Fraction

Mole Fraction (X) represents the mole component by total moles.&nbsp;

Mole Fraction -

The Ideal Gas Law Derivations

The&nbsp;Ideal Gas Law Derivations are a convenient way to solve gas calculations involving 2 sets of the same variables.&nbsp;

Root Mean Square Speed

Root Mean Square Speed&nbsp;allows for the determination of the velocity of 1 type of gas molecule.

The Ideal Gas Law: Density

Under certain conditions of pressure and temperature, the Ideal Gas Law can determine the density&nbsp;of a gas.&nbsp;

Effusion is the escaping of gas molecules or atoms through a pinhole.&nbsp;

Kinetic Energy of Gases

Kinetic Energy is the energy an object possesses due to its motion.

Gas Stoichiometry

Gas Stoichiometry involves chemical reactions that contain gases.

The Ideal Gas Law

The Ideal Gas Law formula relates the behavior of gases under varying conditions of pressure, volume, moles and temperature.

Chemistry Gas Laws: Combined Gas Law

The Combined Gas Law&nbsp;is created from “combining” Boyle’s Law, Charles’ Law, and Gay–Lussac’s Law.

Pressure Units

Pressure is the force that is exerted within a given volume of space.&nbsp;

Kinetic Molecular Theory

A gas is seen as a collection of molecules or individual atoms that are in constant motion. The Kinetic-Molecular Theory tries to use data of real gases to predict how an ideal gas would behave if they existed.&nbsp;&nbsp;

Standard Temperature and Pressure

In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under Standard Temperature and Pressure.&nbsp;

The Ideal Gas Law Applications

The Ideal Gas Law Applications establish both the direct and inverse relationships between the Ideal Gas Law variables.

Maxwell-Boltzmann Distribution

The Maxwell-Boltzmann Distribution is a probability distribution curve that describes the speed of a gas at a specific temperature.

Chemistry Gas Laws

Chemistry Gas Laws&nbsp;are laws that relate together the pressure, volume and temperature of a gas.

The Ideal Gas Law: Molar Mass

The Ideal Gas Law can be further extended to find the molar mass of a gas.&nbsp;

Van der Waals Equation

The&nbsp;Van der Waals Equation is used when dealing with real, non-ideal gases.&nbsp;