Chapter 10: Properties of Gases

Gases

no definite shape or volume. Random arrangement of particles, far apart. weak on no inter-particle interaction

Plasma

"Ionized gas". No definite shape or volume. Unique properties. Flames, fluorescent lights, arc welder, lightening, stars, outer space.

Pressure

arises from collisions of gas particles with walls of its container. Equals force exerted per unit area. P=F/A

Barometer

An instrument that measures atmospheric pressure

PV=nRT

ideal gas law equation. Pressure, Volume in L, temperature in K, number of moles, R gas constant (0.082058 Latm/molK)

Standard Conditions

STP "Standard temperature and pressure". 1 atm pressure. 0 degree Celsius or 273.15 K. 1 mole of an ideal gas occupies 22.414 L (Molar Volume)

Inversely Proportional

At constant temperature and moles of gas, Volume and Pressure are __________________ _____________________.

Boyle's Law

P1V1=P2V2

Directly Proportional

At constant pressure and moles of gas, volume and temperature are ___________ ___________________.

Charles' Law

V1/T1=V2/T2

Gay-Lussac's Law

At constant volume and moles of gas, temperature and pressure are directly proportional. P1/T1=P2/T2

Avogadro's Law

At constant temperature and pressure, moles of gas and volume are directly proportional. V1/n1=V2/n2

Dalton's Law

Ptotal=P1+P2+...

P(total)

depends on the total number of gas particles present

Partial Pressure

pressure exerted by a single gas in a mixture

mole fraction (XA)

unit of concentration where the number of moles of a component is divided by the total number of moles in the mixture. (moles A/total moles)

diffusion

mixing of different gases by random molecular motion and collision

Effusion

when gas molecules escape without collision, through a tiny hole into a vacuum

Graham's Law

the rate of effusion of a gas is inversely proportional to the square root of its molar mass

Low; high

Real Gases deviate significantly from ideal behavior at ______ temperatures and/or _____ pressures.

At high pressure,

volume

At low temperatures,

the observed gas pressure is less than predicted