Gases -ideal law

Solid

Molecules are arranged in regular, repeating patterns and can only vibrate around fixed positions, maintaining a definite shape and volume.

Liquid

Molecules are close together with no definite shape but a definite volume, allowing them to flow and take the shape of their container.

Gas

Molecules are far apart and move freely, resulting in no definite shape or volume, filling the entire space of their container.

Plasma

A state of matter where atoms are ionized, consisting of free electrons and ionized nuclei, typically found at high temperatures, such as in stars.

Ideal gas law

An equation of state for an ideal gas that relates pressure, volume, temperature, and the number of moles, commonly expressed as $PV = nRT$

Ideal gas assumption

1. Negligible size

2. All collisions between gases and the container are frictionless

3. No attractive or repulsive forces

4. Gas molecules are in constant motion

SI units

Kinetic energy equation

ke = ½ mv²

Root mean squared speed

Maxwell Boltzmann distribution

Mass - smaller mass = faster speed = flatter curve

Temperature - lower temperature = shorter steeper curve

Problems with ideal gas vs real gas

Z is the deviation from normal behaviour = z>1 volume is larger but if z<1 the volume is smaller than expected

Better model of PV=nRT

p+a(n/v)² - a describes the intermolecular force, and n/v is the distance that these forces are applicable

v-nb - volume minus the number of gas moles related to the volume

Real Volume

it accounts for the deviation from an ideal gas, it doesn’t include the volume of the actual molecules hence we minus it

Better version of Ideal Gas

It can describe critical temperatures and predict liquid phases