Gases: Video recap – The Kinetic Molecular Theory describes how gas particles behave Gas pressure is the result of particle collisions with the walls of a container or an object.

IM Forces and Gases: What’s the connection? Substances that are gases at cold temperatures tend to be substances with little to no IM forces We define most gases as ideal gases, which assumes that they experience no attractive forces at all!

IM Forces and Gases: What’s the connection? Substances that are liquids and solids (due to stronger IM forces) can be made into gases by adding enough heat to break the IM forces and separate the particles.

Gases: Video recap – The Kinetic Molecular Theory describes how gas particles behave Gas pressure is the result of particle collisions with the walls of a container or an object.

They are always equal

More particles added, collisions increase, but since pressure must stay constant, the volume increases Heating a gas makes them move faster, collisions increase, but since pressure stays constant, the volume increases.

As the external pressure is decreased, the internal pressure will also decrease. The only way for internal pressure to decrease without a change in temperature or particles, is for the volume to increase.

V vs. n V vs. T V vs. P Direct! Direct! Inverse k = k = k =

P = 1 P = 1 V = 1 V = 1 P = 1 V = 2 How does half as many particles give the same P in the same V?

P = 1 P = 1 V = 1 V = 1 T = higher T = lower P = 1 V = 2 T = higher than the 1st

P = 1 P = 1 P = 1 V = 1 V = 1 P = 1 V = 0.5 T = middle T = low V = 2 T = lowest T = highest