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Definition
a. The property that determines the direction of thermal energy transfer between two objects.
b.)A measure of the average random kinetic energy of the particles of a substance. |
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Definition
| two objects are in thermal equilibrium when they are at the same temperature so that there is no transfer of thermal energy between them |
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| *Internal Energy of a substance(U) |
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Definition
| The total potential energy and random kinetic energy of the molecules of the substance. |
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| *Thermal Energy (Heat) (Q) |
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Definition
| Energy transferred between two substances in thermal contact due a temperature difference. |
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| An amount of a substance that contains the same number of atoms as 0.012 kg of 12C. |
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| The mass of one mole of a substance. |
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Definition
| The number of atoms in 0.012 kg of 12C (= 6.02 x 1023). |
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Definition
| energy required to raise the temperature of a substance by 1K |
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| *Specific Heat Capacity (c) |
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Definition
| energy required per unit mass to raise the temperature of a substance by 1K |
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Definition
| a phase change of a liquid into a gas that occurs at a fixed temperature |
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Definition
| when faster moving molecules have enough energy to escape from the surface of a liquid that is at a temperature less than its boiling point, leaving slower moving molecules behind which results in a cooling of the liquid |
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| *Specific Latent Heat (L) |
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Definition
| energy per unit mass absorbed or released during a phase change |
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Definition
| force per unit area acting on a surface |
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Definition
| a gas that follows the ideal gas equation of state (PV = nRT) for all values of P, V, and T (an ideal gas cannot be liquefied) |
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Definition
| a gas that does not follow the ideal gas equation of state for all values of P, V, and T (a real gas can approximate an ideal gas in some circumstances) |
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| Absolute Zero of Temperature |
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Definition
| temperature at which a gas would exert no pressure |
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| Kelvin scale of Temperature |
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Definition
| an absolute scale of temperature in which 0 K is the absolute zero of temperature |
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| *First Law of Thermodynmaics (U = ΔU + W) |
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Definition
| The thermal energy transferred to a system from its surroundings is equal to the work done by the system plus the change in internal energy of the system. (an application of the principle of conservation of energy) |
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| Isochoric (Isovolumetric) |
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Definition
| a process that occurs at constant volume (ΔV = 0) |
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Definition
| a process that occurs at constant pressure (ΔP = 0) |
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Definition
| a process that occurs at constant temperature (ΔT = 0) |
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Definition
| a process that occurs at constant temperature (ΔT = 0) |
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Definition
| a system property that expresses the degree of disorder in the system |
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| *Second Law of Thermodynamics |
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Definition
| The overall entropy of the universe is increasing. (OR – All natural processes increase the entropy of the universe.) (NOTE: The second law implies that thermal energy cannot spontaneously transfer from a region of low temperature to a region of high temperature.) |
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