gas laws, SI units for gas laws, real gas? ideal gas? real -> ideal gas

Avogadro’s Law

V ∝ n

Gay-Lussac’s Law

P ∝ T

Charles’ Law

V ∝ T

Boyle’s Law

P ∝ 1/V

Combined Gas Equation

P₁V₁/T₁ = P₂V₂/T₂

Ideal Gas Equation

PV = nRT, where R is ideal gas constant

Pa

SI of pressure

pressure

the amount of force a gas exerts on the walls of a container per unit area.

bar

100kPa

m³

SI of volume

K

SI of temperature

temperature

a consequence of molecular motion

ideal gas has (4)

no IMFs (non-interacting particles)
point molecules, points with no volume
in a constant state of random linear motion
collide elastically (don’t lose KE when colliding with anything)

real gas (4)

IMFs
occupy molecular volume
constant state of random linear motion
collides inelastically (KE & thus speed is lost)

real → ideal gas (3 = 2 (combined) + 1)

increase temperature to increase KE to increase speed to weaken IMFs, and also make any KE loss from collisions negligible
lower pressure to reduce number of molecules so the gas occupies less molecular volume

SLC and STP special aspect (2)

P is low enough, T is high enough for ideal gas assumptions to hold

P = ?

F/A

T = ?

c * ½ * mv²

1 atm

101.32kPa

torr

1mmHg or 0.133322 kPa (6s.f.)