HONORS CHEMISTRY REVIEW TOPICS

CHAPTER 10 – “Gases”

Characteristics of gases

Pressure = force/area in N/m² or pascal (Pa)

Force=mass x acceleration due to gravity, F=mA

Measuring pressure - barometer, manometer

Standard pressure in mm Hg, torr, atmospheres. Pascals or KPa (know values)

Standard Temperature and Pressure:  STP (know units and values)

Direct and inverse relationships

Gas Laws

Boyle's Law PV=k or P₁V₁ = P₂V₂

Charles Law: V/T = k or V₁/T₁ = V₂/T₂  Kelvin temperature, absolute zero

Gay-Lussac’s Law of combining volumes

Avogadro's Law: V/n = k

Combined law: P₁V₁/n₁T₁ = P₂V₂/n₂T₂

Ideal gas equation PV = nRT where R = gas constant

Molar volume = 22.4liters at STP

Density of gases at various conditions.

Applications of gas laws:

Volume-volume stoichiometry

Mass-gas volume stoichiometry

Dalton’s Law of Partial Pressure

Mole Fraction

Kinetic Molecular Theory (know the 5 statements – p. 414)

Graph of kinetic energy of gases: Average K.E. vs. # of molecules

Average kinetic energy of gases: ε = ½ mυ²

Ideal vs. real gases (sizes and forces)