Gases

Please login.

This is a 8 point assignment

Objectives: After completing this unit, students should be able to:

1. Describe how a barometer and manometer can be used to measure gas pressure.
2. Convert among various units of pressure, including torr, atmosphere, mm of Hg, and Pascals.
3. Solve problems using Boyle’s law, Charles’ law, the combined gas law, and Avogadro’s Law.
4. Solve problems using the ideal gas law.
5. Know the value of STP.
6. Starting with the ideal gas law, derive a relationship that includes molar mass and gas density and then solve problems using it.
7. Using a balanced equation, convert from a given mass, mole, or volume of one gas phase substance to mass, mole, or volume of another.
8. Solve problems using Dalton’s Law of Partial Pressures.
9. Calculate the mass of a reactant given the volume, total pressure, and temperature of a gas collected over water.
10. List and explain the principle points of the kinetic molecular theory of gases and describe the factors responsible for real gases deviating from ideal gases.
11. Describe the relationship between temperature, average velocity, and kinetic energy.
12. State Graham’s law and use it to solve problems.
13. Explain the origin of the correction terms to P and V that appear in the Van der Waal’s equation.

Reading and Homework Exercises

Table of Contents from: OpenStax Chemistry 2e: Chapter 9

Introduction

9.1 Gas Pressure

Questions 1 and 2 check your ability to convert between some common units of pressure and test your understanding of a barometer (which is used to measure ambient atmospheric pressure).

Question 1:

Question 2:

9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law

Questions 3-11 test your understanding of various gas laws and  check your ability to solve gas law problems.

Question 3:

Question 4:

Question 5: Answer the following question for the gas phase decomposition of dinitrogen pentoxide:

2 N₂O₅ –> 2 N₂ + 5 O₂

Question 6:

Question 7:

Question 8:

Question 9:

Question 10:

Question 11:

9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions

Questions 12 and 13 test your understanding of the relationship of the ideal gas law, gas density, and molar mass of a gas and to use these relationships to solve problems

Question 12:

Question 13:

Questions 14 and 15 test your ability to solve stoichiometry problems involving gases

Question 14: Aluminum oxide is decomposed as follows:

2 Al₂O₃ (s) → 4 Al (s) + 3 O₂ (g).  Answer the following question given this reaction.

Question 15: Lithium nitride, Li₃N, is decomposed as follows:

2 Li₃N → 6 Li + N₂

Answer the following question:

Questions 16 -20 test your understanding of what happens when gases mix and Dalton’s Law of partial pressure

Question 16:

A tank contains a mixture of three gases (nitrogen, oxygen, and helium), each with the partial pressure as shown in the figure below:

Answer the following two questions (all with the correct number of significant figures) given the above figure:

Question 17:

Question 18:

Question 19:

Question 20:

9.4 Effusion and Diffusion of Gases and

9.5 The Kinetic-Molecular Theory

Questions 21-24 test your understanding of the priciples you have learned about the Kinetic Molecular Theory of gases

Question 21:

A tank contains a mixture of three gases: N₂, O₂, and He.  Answer the following three questions for this mixture:

Question 22:

Question 23:

Question 24:

Questions 25-27 test your understanding of effusion and Graham’s Law

Consider separate 1.0 L gas samples of NH₃, H₂, CO₂, N₂O₅, CCl4.  Answer the following question:

Question 25:

Question 26:

Question 27:

9.6 Non-Ideal Gas Behavior

Questions 25-27 test your understanding of the conditions that make a gas behave more (or less) like an ideal gas.

Question 28:

Question 29:

Question 30: