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

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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.

ð 1 mole of any gas at STP=22.4 L

ð 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.

ð Avogadro’s law (n/V=k), n₁/V₁ = n₂/V₂

ð Dalton’s law (P_T=P₁+P₂+P₃ ...)

ð Vapor pressure of water as a function of temperature (conceptually).