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28 Cards in this Set
- Front
- Back
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How to convert Kelvin to Celsius.
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K - 273 = C
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Thermal energy naturally flows from:
A) Hot to Cold B) Cold to Hot |
A) Hot to Cold
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Thermal equilibrium
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When two objects have experienced a transfer of thermal energy such that both now have the same temperature.
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Mole
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The SI unit for 'amount of substance'. One mole of a substance is equal to the amount of that substance that contains the same number of atoms as 0.012kg of carbon-12.
One mole is 6.02 x 10^23 |
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Molar Mass
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The mass of one mole of a substance. If an element has a certain mass number, A, then the molar mass will be A grams.
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Microscopic View
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Looks inside the system to see how its component parts interact with each other.
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Macroscopic View
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Considers the system as a whole and sees how it interacts with its surroundings.
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Internal Energy
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The total energy that the molecules of a substance possess (kinetic plus potential)
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Temperature
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A measure of the average kinetic energy of the molecules in a substance.
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Potential energy of molecules in a substance can be attributed to what?
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Intermolecular forces.
Pulling two molecules further apart, for example, would require work against intermolecular forces. |
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Kinetic energy of molecules in a substance can be attributed to what?
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The movement of the molecules.
Molecules can have either translational kinetic energy (moving in a certain direction) or rotational kinetic energy (rotating about one or more axes). |
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Thermal Capacity
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The energy required to raise a substance's temperature by 1 Kelvin.
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Specific Heat Capacity
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The energy require to raise a unit mass of a substance by 1 Kelvin.
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Formula for Thermal Capacity (C)
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C = Q / ΔT
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Formula for Specific Heat Capacity (c)
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c = Q / (m ΔT)
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If two solids of different temperature are placed in contact with each other such that no heat is lost to the environment, what is the ratio of the energy lost by the hot substance to the energy gained by the cold substance?
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1 : 1
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Latent Heat
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The amount of energy associated with a phase change.
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Specific Latent Heat
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The amount of energy per unit mass absorbed or released during a change of phase.
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Formula for Specific Latent Heat (L)
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L = Q / m
L = Joules / kilogram |
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Does the rate of evaporation depend on the surface area of the liquid?
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Yes.
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Does the rate of evaporation depend on the mass of the liquid?
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No.
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Does the rate of evaporation depend on the temperature of the liquid?
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Yes. As temperature increases, the rate of evaporation increases.
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Does the rate of evaporation of a liquid depend on the pressure of the surrounding air?
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Yes. As pressure increases, evaporation rate decreases.
This occurs because as pressure increases, the boiling point increases. |
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Kinetic Model of an Ideal Gas
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Assumptions:
-Newton's laws apply to molecular behavior -There are no intermolecular forces -The molecules are treated as points -The collisions between molecules are elastic (no energy is lost) -There is no time spent in these collisions |
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Pascal
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Newton per meter squared, the SI unit for pressure.
Pressure = Force / Area |
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Pressure Law (Gay-Lussac's Law)
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At a constant volume, the pressure of a gas is proportional to its temperature in Kelvin.
P = k*T |
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Charles's Law
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At a constant pressure, the volume of a gas is proportional to its temperature.
(V1) / (T1) = (V2) / (T2) OR V = k*T |
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Boyle's Law
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At a constant temperature, the pressure of a gas is inversely proportional to its volume.
(P1)(V1) = (P2)(V2) OR P = k/V |
