Gasses Honors Chemistry

Kinetics/molecular theory

Helps explain behavior of states of matter (matter is made of particles in constant motion, particles move straight until collision and no energy is lost from collision, particles are small, particles aren’t attracted or repelled, kinetic energy depends on temp)

Diffusion

Results from the mixing of multiple gases (Smell from food getting into O2 in the air)

Kinetics/molecular theory

Helps explain behavior of states of matter (matter is made of particles in constant motion, particles move straight until collision and no energy is lost from collision, particles are small, particles aren’t attracted or repelled, kinetic energy depends on temp)

Diffusion

Results from the mixing of multiple gases (Smell from food getting into O2 in the air)

Effusion

Gas particles escape through small opening (O2 leaking from tire)

Gas properties

Particles are spread, indefinite volume/shape, particles move freely (fluid), most volume is empty space, highly compressible.

STP

Standard pressure/ temp = 1 atm (0 degrees Celsius) 273k

Pressure

Force exerted per unit of area due to the collisions of particles. Measured with a barometer. 1 atm=760 mmHg=760 torr=101.325 kPa

Four qualities of gas

Pressure, temperature, volume, amount of gas (mol)

Temperature

Measure of kinetic energy of particles in matter. Kelvin must be used in any gas law equations!! Absolute zero is where all motion stops.

Boyle’s Gas Law

States that volume and pressure are inversely proportional at a constant temperature meaning that as pressure increases volume decreases and likewise. P1V1=P2V2

Charle’s Gas Law

States that at a constant pressure volume and temperature are directly proportional meaning that as temperature increases so does volume. V1/T1=V2/T2

Gay Lussac’s Gas Law

States that at a constant volume pressure and temperature are directly proportional meaning that as temperature increases so does pressure. P1/T1=P2/T2

Avogadro’s Gas Law

States that at a constant temperature and pressure volume and number of moles are directly proportional meaning that as number of gas moles increases so does volume. V1/N1=V2/N2

Combined Gas Law

States that pressure and volume are inversely related to each other and both related to temperature. P1V1/T1=P2V2/T2.

Dalton’s Law of Partial pressure

States that the total pressure of a combined gas is equal to the sum of each of the combined gasses partial pressure. P(total)= P1+P2+P3…

Ideal Gas Law

Describes the behavior of an ideal gas for any combination of pressure/moles/volume/temperature. PV=nRT R= 0.0821 P= atm V= L n= moles T= temperature in Kelvin.

Graham’s Law of Effusion

The rate at which effusion occurs is inversely proportional to the square root of its molar mass. Rate1/Rate2= (square root MM2)/(Square root MM1).