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18 Cards in this Set
- Front
- Back
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Thermodynamics
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The study of the flow of heat and thermal energy
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Total Energy
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Total Energy = Internal + Kinetic + Potential
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Temperature
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Measure of the average kinetic energy of the molecules of a substance.
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Heat
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Internal energy exchanged by two bodies in contact.
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Ideal Gas Law
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PV=nRT
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Average Kinetic Energy of a Gas
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K=3/2(boltzman's constant)*Temperature (K)
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Internal Energy of a System (U)
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The sum of all kinetic energies of all the molecules of a system.
U=NK(ave) U=N*3/2*(Boltzman's constant)(Temperature) |
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First Law of Thermodynamics
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Change in energy = heat flow into system + work done on the system
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Directions of Heat and Work
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Heat flowing from the environment to the system is positive heat.
Work done by the surrondings on the system is positive work. |
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Thermodynamic State
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The state of a gas defined by its pressure, volume, and temperature.
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Isothermal Process
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A process in which the temperature (and therefore the internal energy of the system) remains constant.
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Isobaric Process
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A process in which the pressure is constant.
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Isometric Process
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Constant volume. Also known as isochoric process. Since there is not change in volume, no work is done on the gas.
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Adiabatic Process
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A process that happens with no change in heat with the outside surroundings. Since Q = is zero, then
delta-U=W |
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Work done on a gas
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W=-P*(delta)V
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When a gas completes a cycle
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There is no change in temperature or internal energy of the system.
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Heat Engines
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Convert heat into work. This process is never 100% efficient.
Heat flows from a region to Qh to a region of lower temperature Ql. The work is Qh-Ql. |
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Efficiency of a heat engine.
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e=Work/Qh
or e= (Th-Tl)/Th |
