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| 3 things about the kinetic theory of matter? |
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Definition
a. Assumes that all the particles in a substance are in constant motion
b. State of matter is determined by amount of motion and spacing between particles
c. Temperature is the measure of the average kinetic energy in a substance |
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| the measure of the average kinetic energy in a substance |
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| Compare the three common states of matter in terms of the kinetic theory. |
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Definition
a. Solid: particles are closely packed and vibrating slightly
b. Liquid: particles are further apart than solids; slip and slide around
c. Gas: particles are very far apart and zip around |
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| a. Diffusion: the movement of particles from areas of high concentration to low concentration. Effusion: diffusion of a gas out of its container |
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| a force per unit area exerted by the collision of gas particles against the side of its container |
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| Graham's Law of Effusion equation |
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Definition
| rate A/rate B = square root MB / square root MA |
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| Torricelli measured the height of a column of mercury that was in equilibrium with gravity. 760 mm Hg |
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| Dalton's law of partial pressures |
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Definition
| a. The total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas. |
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SI unit for pressure
101.3 kPa |
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standard temperature and pressure.
set of environmental conditions by which we can compare gases.
0 degrees C, 1 atm.
(273 K and 101.3 kPa) |
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| force of attraction created by the collision of two molecules which induces a dipole. weakest force. |
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| when 2 polar molecules are attracted to each other |
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| same as dipole-dipole, but one of the atoms is Hydrogen |
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Definition
| ability to flow. also applies to gases |
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| resistance to flow. inversely proportional to temperature |
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| much higher than gases. much less compressible. |
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| attraction of particles toward the center of a liquid |
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| substance that disrupts surface tension |
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| tendency for a liquid to stick to the sides of its container |
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| density of solids is ______________ than liquids |
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| particles are arranged in a repeating geometric pattern |
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| simplest unit of the crystalline solid |
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| all sides equal, all angles 90 |
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| 2 sides equal, all angles 90 |
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| no sides equal, all angles 90 |
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| all sides equal, all angles equal, no angles 90 |
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| multiple unit cells together |
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| particles arranged randomly. aka supercooled liquids because they exhibit flow. |
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| removal of all energy from liquid causes the particles to slow down and get closer. freezing pt water: 0 |
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| increase in energy causes particles to move faster and spread apart. melting pt water: 0 |
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| amount of energy needed to convert 1 mol from liquid to solid (or vice versa) at its melting/freezing point |
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Definition
| transition from liquid to gas |
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| molecules on the surface of the liquid gain enough energy to break off from the rest of the liquid. can happen at room temperature |
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| vapor pressure of the liquid must exceed the atmospheric pressure. boiling pt water: 100 |
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| transition from gas to liquid. condensation pt: 100 |
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| molar heat of vaporization |
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Definition
| the amount of energy needed to convert 1 mol of any liquid to a gas at its boiling temperature. applies to vaporization and condensation |
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| transition from solid to gas |
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| gas to solid without going through liquid |
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| temperature and pressure at which all three states of matter are in equilibrium |
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| critical temperature and pressure of a substance |
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| temperature beyond which no amount of pressure can force a gas back into a liquid |
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| when a substance is at its critical temperature, it is the minimum amount of pressure needed to make it a liquid |
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