Particles in all forms of matter are in constant motion, kinetic energy of a substance is directly proportional to the temperature of substance, temperature is a measure of an object's average kinetic energy, all items at same temp = same KE

Unit of temperature that measures amount of kinetic energy

Gas particles are small spheres with insignificant volume, gas particles move rapidly in contact random motion, all collisions are perfectly elastic, no transfer/loss, there is not attraction or repulsion between particles

Gas pressure is defined as the force exerted by a gas per unit of surface area, gas pressure is caused by millions of collision of the gas particles with the side of the container

1 atm, 760 mmHG, 760 torr, 101.3kPa

Occurs at surface of liquid, cooling process since KE decreases

Gas trapped above a liquid, increased with increasing temperature, and more evaporation = higher.

When you heat a liquid, more particles leave the surface and increased vapor pressure, vapor pressure = external pressure , normal boiling point is 1 arm

P1 x V1 = P2 x V2, inversely related, only when constant.

V1 = V2, directly related, temperature must be in Kelvin T1 = T2

P1 = P2, directly related, only if held constant, must be in Kelvin T1 = T2

V1 = V2,If two samples of a gas at STP have the same volume, they contain the n1 = n2 same number of molecules, directly related only if held constant.

P1V1 = P2V2 hard to keep constant, use when something is changing, n1T1 = n2T2

Have atoms that take up negligible space, doesn't have IMF attractions, move randomly and have perfectly elastic collisions, low temp and high pressure is not ideal, ideal gasses are close to STP and don't change PvNRT

Dalton's Law of Partial Pressures

When you have a mixture of gases the total pressure of the system will be equal to the sum of partial pressure of each of the individual gases.

Diffusion - gas particles moving from high to low concentration Effusion - gas particles moving from high pressure to low pressure. Graham states that heavy gases move slow and lighter gases move quickly

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Chem Unit !

Term	Definition
Vaporization/Boiling	Liquid to gas
Condensing	Gas to liquid
Sublimation	Solid to gas
Deposition	Gas to solid
Kinetic theory	Particles in all forms of matter are in constant motion, kinetic energy of a substance is directly proportional to the temperature of substance, temperature is a measure of an object's average kinetic energy, all items at same temp = same KE
Kelvin Scale	Unit of temperature that measures amount of kinetic energy
Nature of Gases	Gas particles are small spheres with insignificant volume, gas particles move rapidly in contact random motion, all collisions are perfectly elastic, no transfer/loss, there is not attraction or repulsion between particles
Gas Pressure	Gas pressure is defined as the force exerted by a gas per unit of surface area, gas pressure is caused by millions of collision of the gas particles with the side of the container
Pressure Units	1 atm, 760 mmHG, 760 torr, 101.3kPa
Evaporation	Occurs at surface of liquid, cooling process since KE decreases
Vapor Pressure	Gas trapped above a liquid, increased with increasing temperature, and more evaporation = higher.
Boiling Point	When you heat a liquid, more particles leave the surface and increased vapor pressure, vapor pressure = external pressure , normal boiling point is 1 arm
Boyle's Law	P1 x V1 = P2 x V2, inversely related, only when constant.
Charles' Law	V1 = V2, directly related, temperature must be in Kelvin T1 = T2
Gay-Lussac's Law	P1 = P2, directly related, only if held constant, must be in Kelvin T1 = T2
Avogadro's Law	V1 = V2,If two samples of a gas at STP have the same volume, they contain the n1 = n2 same number of molecules, directly related only if held constant.
Combined Gas Law	P1V1 = P2V2 hard to keep constant, use when something is changing, n1T1 = n2T2
Ideal Gases	Have atoms that take up negligible space, doesn't have IMF attractions, move randomly and have perfectly elastic collisions, low temp and high pressure is not ideal, ideal gasses are close to STP and don't change PvNRT
Dalton's Law of Partial Pressures	When you have a mixture of gases the total pressure of the system will be equal to the sum of partial pressure of each of the individual gases.
Graham's Law	Diffusion - gas particles moving from high to low concentration Effusion - gas particles moving from high pressure to low pressure. Graham states that heavy gases move slow and lighter gases move quickly

Created by: Armyyy

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