Gases Chemistry Worksheet - Chapter 13, An Introduction To Chemistry Page 34
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Chapter 13
Gases
Chapter
Ideal gas model The model for gases that assumes (1) the particles are point-masses
(they have mass but no volume) and (2) there are no attractive or repulsive forces
Glossary
between the particles.
Ideal gas A gas for which the ideal gas model is a good description.
Pressure Force per unit area.
Boyle’s Law The pressure of a gas is inversely proportional to the volume it occupies
if the number of gas particles and the temperature are constant.
Gay-Lussac’s Law The pressure of an ideal gas is directly proportional to the Kelvin
temperature of the gas if the volume and the number of gas particles are constant.
Charles’ Law Volume and temperature are directly proportional if the number of gas
particles and pressure are constant.
Avogadro’s Law Volume and the number of gas particles are directly proportional if
the temperature and pressure are constant.
Universal gas constant, R The constant in the ideal gas equation.
Partial pressure The portion of the total pressure that one gas in a mixture of gases
contributes. Assuming ideal gas character, the partial pressure of any gas in a
mixture is the pressure that the gas would yield if it were alone in the container.
Dalton’s Law of Partial Pressures The total pressure of a mixture of gases is equal to
the sum of the partial pressures of each gas.
You can test yourself on the glossary terms at the textbook’s Web site.
Chapter
The goal of this chapter is to teach you to do the following.
Objectives
1. Define all of the terms in the Chapter Glossary.
Section 13.1 Gases and Their Properties
2. For a typical gas, state the percentage of space inside a gas-filled container that is
occupied by the gas particles themselves.
3. State the average distance traveled between collisions by oxygen molecules, O
, at
2
normal room temperature and pressure.
4. Write the key assumptions that distinguish an ideal gas from a real gas.
5. Describe the process that gives rise to gas pressure.
6. State the accepted SI unit for gas pressure.
7. Convert between the names and abbreviations for the following pressure units:
pascal (Pa), atmosphere (atm), millimeter of mercury (mmHg), and torr.
8. Convert a gas pressure described in pascals (Pa), atmospheres (atm), millimeters
of mercury (mmHg), or torr to any of the other units.
9. Convert between the names and variables used to describe pressure (P),
temperature, (T ), volume (V ), and moles of gas (n).
10. For each of the following pairs of gas properties, describe the relationship
between the properties, describe a simple system that could be used to
demonstrate the relationship, and explain the reason for the relationship:
(a) volume and pressure when the number of gas particles and temperature are
constant, (b) pressure and temperature when volume and the number of gas
particles are constant, (c) volume and temperature when pressure and the number
of gas particles are constant, (d) the number of gas particles and pressure when
volume and temperature are constant, and (e) the number of gas particles and
volume when pressure and temperature are constant.
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