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| Goal
I. Identify and relate the variables which describe the state of a gaseous
system. |
Objectives: To meet the requirements of Goal
I, you must be able to:
-
define the
state variable pressure, and explain how a mercury barometer
measures atmospheric pressure;
-
convert among
the pressure units mmHg (torr) atmospheres, pascals,
and kilopascals;
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explain
the concept of the volume of a gas and how it differs from the volume of
a solid or a liquid;
-
solve Boyle's
Law problems relating
changes in the volume of a gas to changes in its pressure when temperature
and the amount of sample remain constant;
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solve Charles'
Law problems relating
changes in the volume of a gas with changes in its absolute temperature
when pressure and amount of sample remain constant;
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describe
how the value of "absolute zero" can be determined using Charles'
Law;
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solve combined
Boyle's Law and Charles' Law problems relating to changes in pressure,
temperature and volume;
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know the
pressure and temperature conditions known as STP (Standard
Temperature and Pressure) for gases;
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relate
volume to number of gas particles (Avogadro's Law) when temperature and
pressure are held constant; apply
Gay-Lussac's Law for combining volumes;
-
use the ideal gas
law to find:
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P,V, n or T given three of the four quantities
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volume of a gas used or formed
in a chemical reaction
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the density of a gas
-
the molecular mass of a gas. [Top]
| Goal II. Apply Dalton's
Law of Partial Pressure to mixtures of gases. |
Objectives: To meet the requirements of Goal
II, you must be able to:
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write the expression
for the total pressure for any mixture of gases using Dalton's Law of
Partial Pressure;
-
use Dalton's
Law of Partial Pressure to calculate:
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the partial pressure of a gas in a mixture of gases
and the total pressure of the mixture
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the dry volume of a gas collected
over water.[Top]
| Goal III. Use the kinetic-molecular
theory as a model to explain the behavior of gases. |
Objectives: To meet the requirements of Goal
III, you must be able to:
-
interpret Figure
5.14 (p. 200) and Figure 5.19 (p. 203) using the kinetic-molecular theory
of gases to explain the concepts of distribution of molecular speeds,
average molecular speed, and the dependence of the distribution and average
of molecular speeds on temperature; relate
average molecular speed to mass of gas particles;
-
explain Boyle's
Law and Charles' Law in terms of the kinetic-molecular theory;
-
compare and contrast
real gases and ideal gases and use the kinetic-molecular theory to explain
the conditions under which a real gases exhibits behavior similar to that
of an ideal gas. [Top]
|
Unit 5 Assignments
|
| Read: |
Text
Chapter 5, pp. 176-213 |
| Video
Programs: |
- Kinetic
Molecular Theory
- Gas
Laws, Ideal Gas Law
- Gas
Stoichiometry, Molar Volume, Density
|
| Textbook
Assignments: |
Read
and Understand all "Sample Problems," "Follow
Up Problems" and the blue-colored problems at the
end of the chapters.
The
answers for the Follow Up Problems are at the end
of the chapter; the answers for the blue-colored
problems are in Appendix C.The answers for each
of these are in Appendix C.
|
| ChemSkill
Builder Assignments: |
Mandatory
assignments to be submitted for grade
Chapter 7, Sections
7.1, 7.2, 7.3, 7.4 and 7.5
|
| Note:
Complete Solutions, including all units of measurement,
must be shown for all problems. |
[Top]
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