UNIT 10 – GASES
I. Kinetic-Molecular Theory
B. Ideal Gases
II. Ideal Gas Equation
1. Molar Mass
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
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).