UNIT 10 –
GASES
I. Kinetic-Molecular Theory
A. Assumptions
B. Ideal Gases
C. Conversions
1. Pressure
2. Temperature
3. Volume
4. Quantity
II. Ideal Gas Equation
A.
Calculations
B.
Applications
1.
Molar Mass
2.
Density
III. Gas Laws
A.
Combined Gas
Law
B.
Boyle’s Law
C.
Charles’ Law
D.
Gay-Lussac’s
Law
IV. Gas Stoichiometry
A.
Molar Volume
B.
Different
types of problems
V. Other Gas Information
A. Dalton’s Law of Partial Pressure
B. Graham’s Law of Effusion
North Carolina Essential
Standards and Clarifying Objectives:
Chm. 2.1 Understand the
relationship among pressure, temperature, volume, and phase.
2.1.5 Explain the
relationships among pressure, temperature, volume, and quantity of gas,
both qualitative
and quantitative.
•
Identify
characteristics of ideal gases.
•
Apply the
following formulas and concepts of kinetic molecular theory.
š
1 mole of
any gas at STP=22.4 L
š
Ideal gas
equation (PV=nRT), Combined gas law (P1V1/T1 =
P2V2/T2) and applications holding one variable
constant: for PV=k,
P1V1 = P2V2;
for V/T=k, V1/T1= V2/T2; for P/T=k,
P1/T1 = P2/T2. Note: Students
should be able to derive and use these gas laws,
but are not necessarily
expected to memorize their names.
š
Avogadro’s
law (n/V=k), n1/V1 =
n2/V2
š
Dalton’s law
(PT=P1+P2+P3 ...)
š
Vapor
pressure of water as a function of temperature (conceptually).