MCAT Physics Ch 3
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| Zeroth Law of Thermodynamics | Objects are in thermal equilibrium when they are at the same temperature, and experience no net exchange of heat energy.
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| Temperature | Qualitative measure of how hot or cold an object is. This is related to the average kinetic energy of the particles that make up a substance.
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| Thermal Expansion | Describes how a substance changes in length or volume as a function of the change in temperature.
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| Thermodynamic System | Portion of the universe we are interested in observing
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| Surroundings | Everything that is not a part of a system
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| Isolated Systems | Systems that do not exchange matter or energy with the surroundings.
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| Closed Systems | Systems that exchange energy but not matter with their surroundings.
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| Open Systems | Systems that exchange both energy and matter with their surroundings.
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| State Functions | Functions that are pathway independent and are not defined by a process. Ex: Pressure, density, temperature, volume, enthalpy, internal energy, Gibbs free energy, and entropy.
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| Process Functions | Describe the pathway from one equilibrium state to another. Ex: Work and heat
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| First Law of Thermodynamics | Statement of conservation of energy in which the total energy in the universe can never decrease or increase.
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| Note About Internal Energy In A Closed System | Total internal energy is equal to the heat flow into a system minus work done by the system.
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| Heat | Process of energy transfer between two objects at different temps that occurs until the two objects come into thermal equilibrium
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| Specific Heat | Amount of energy necessary to raise 1 gram of a substance by 1 degree C or 1 unit Kelvin.
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| Specific heat of water | 1 cal/g*K
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| Heat Of Transformation | Heat during a phase change which causes a particles's potential energy and energy distribution (entropy) but not kinetic energy.
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| Isothermal Processes' Constant Variable | Temp. is constant and change in internal energy is 0.
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| Adiabatic Processes' Constant Variable | Not heat is exchanged.
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| Isobaric Processes' Constant Variable | Pressure is held constant.
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| Isovolumetric (isochoric) Processes | Volume is held constant and work done by or on the system is 0.
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| Second Law of Thermodynamics | In a closed system, including the universe, energy will spontaneously and irreversibly go from being localized to being spread out (dispersed).
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| Entropy | Measure of how much energy has spread out or how spread out energy has become.
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| Note About Increasing Microstates | As the number of available microstates increases, the potential energy of a molecule is distributed over that larger number of microstates, increasing entropy.
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| Note About Natural Processes And Reversibility | Every process is ultimately irreversible. Under highly controlled conditions, certain equilibrium processes such as phase changes can be treated as essentially reversible.
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| Farenheit Equation | F = 9/5C + 32, K= C + 273
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| Thermal Expansion Equation | Del. L = alpha*L*Del.T
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| Volume Expansion Equation | Del. V = Beta*V*DelT
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| First Law of Thermodynamics | Del. U = Q - W
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| Heated Gained Or Lost (With Temperature Change) | q = mcDel.T
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| Heat Gained Or Lost (Phase Change) | q = mL
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| Entropy and Heat | Del. S = Qrev. / T
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| Second Law Of Thermodynamics | Del.S Universe = Del. S System + Del. S Surroundings > 0
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