Gases Brainstorm:):):):):):):) (Partial Pressure (Dalton's Law of…
Pressure increases inversely with volume
As the temperature increases, the volume increases and vice versa
V1/T1 = V2/T2
As the temperature of a gas increases, the pressure increases
P1/T1 = P2/T2
For any type of gas, if they have the same volume, temperature and pressure they have the same number of particles
Ideal Gas Law
Combined Gas Law
Combines Charle's Law, Boyle's Law, and Guy Lussac's Law
In a container with multiple gases, each type of gas particle exerts a different pressure on the container walls. The total pressure in a container is equal to the pressure of gas a + pressure gas b+ ..... depending on how many gases. The pressure from a particular gas only results from the particles of that particular gas. So the pressure imparted by only gas A is equal to the number of moles of only gas A times the absolute temperature times the gas constant divided by the volume.
Dalton's Law of Partial Pressure
Ptotal = P1+P2+P3+...
Ptotal = ntotal(RT/V)
Kinetic Molecular Theory
The individual particles can be assumed to be negligible (zero)
The constant motion of the particles with the walls of the container cause the pressure exerted by the gas.
The particles don't attract or to repel each other, there are no forces between them.
The average kinetic energy of gas particles has a direct relationship to the Kelvin temperature of the gas.
1.0 atm, 273K
Gas Stoich @ STP: 1 mole = 22.4 L Not at STP...use PV=nRT
760 torr = 760 mmHg = 1.0 atm = 101,325 Pa
Effusion vs Diffusion: Diffusion is when particles moving from an area of high concentration to an area of low concentration. Effusion is when gas particles in random motion move through a small hole.