States of Matter-Gases

Review Packet

Objectives:

• Perform calculations with gas laws: Boyle’s, Charles’, Avogadro’s, Combined, and Ideal
• Perform calculations with the ideal gas law to find the density of a molar mass of the gas
• Interpret or draw graphical relationships between gas variables
• Perform stoichiometric calculations for reaction which produce gases
• Perform calculations with molar volume
• Perform calculations with Dalton’s Law for a mixture of gases
• Perform calculations for gases collected over water
• Perform calculations with rates of effusion to find the molar mass
• Perform calculations with root mean square velocity
• Compare real gases to ideal gases
• Deviations from ideal gas behavior
• Kinetic Molecular Theory

Chapters 1 and 5

Equations and Constants (on yellow sheet)

PV = nRT (P + (n²a)/V²)(V – nb) = nRT

P_A = P_Total x Χ_A P_Total = P_A + P_B + P_C + …

n = m / M K = °C + 273

P₁V₁/T₁ = P₂V₂/T₂ D = m/V

u_rms = √ (3 kT/m) = √(3RT/M) KE per molecule = ½ mv²

KE per mole = (3/2) RT r₁/r₂ = √ (M₂/M₁)

Notes

I. Background – Units of Measure

A. Temperature

B. Volume

C. Pressure

II. Gas Laws

A. Boyle’s Law

B. Charles’s Law

C. Avogadro’s Law

D. Combined Gas Law

E. Ideal Gas Law

F. Gas Density

G. Dalton’s Law of Partial Pressure

III. Kinetic-Molecular Theory

A. Postulates

B. Kinetic Energy of a Gas Sample

C. Root mean square velocity

D. Graham’s Law of Effusion

E. Deviations from ideal gas