Chem Unit !
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| Vaporization/Boiling | Liquid to gas
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| Condensing | Gas to liquid
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| Sublimation | Solid to gas
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| Deposition | Gas to solid
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| 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
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| Kelvin Scale | Unit of temperature that measures amount of kinetic energy
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| 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
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| 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
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| Pressure Units | 1 atm, 760 mmHG, 760 torr, 101.3kPa
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| Evaporation | Occurs at surface of liquid, cooling process since KE decreases
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| Vapor Pressure | Gas trapped above a liquid, increased with increasing temperature, and more evaporation = higher.
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| 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
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| Boyle's Law | P1 x V1 = P2 x V2, inversely related, only when constant.
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| Charles' Law | V1 = V2, directly related, temperature must be in Kelvin
T1 = T2
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| Gay-Lussac's Law | P1 = P2, directly related, only if held constant, must be in Kelvin
T1 = T2
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| 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.
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| Combined Gas Law | P1V1 = P2V2 hard to keep constant, use when something is changing,
n1T1 = n2T2
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| 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
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| 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.
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| 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
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