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MCAT Physics Ch 3
| Question | Answer |
|---|---|
| Zeroth Law of Thermodynamics | Objects are in thermal equilibrium when they are at the same temperature, and experience no net exchange of heat energy. |
| 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. |
| Thermal Expansion | Describes how a substance changes in length or volume as a function of the change in temperature. |
| Thermodynamic System | Portion of the universe we are interested in observing |
| Surroundings | Everything that is not a part of a system |
| Isolated Systems | Systems that do not exchange matter or energy with the surroundings. |
| Closed Systems | Systems that exchange energy but not matter with their surroundings. |
| Open Systems | Systems that exchange both energy and matter with their surroundings. |
| 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. |
| Process Functions | Describe the pathway from one equilibrium state to another. Ex: Work and heat |
| First Law of Thermodynamics | Statement of conservation of energy in which the total energy in the universe can never decrease or increase. |
| 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. |
| Heat | Process of energy transfer between two objects at different temps that occurs until the two objects come into thermal equilibrium |
| Specific Heat | Amount of energy necessary to raise 1 gram of a substance by 1 degree C or 1 unit Kelvin. |
| Specific heat of water | 1 cal/g*K |
| Heat Of Transformation | Heat during a phase change which causes a particles's potential energy and energy distribution (entropy) but not kinetic energy. |
| Isothermal Processes' Constant Variable | Temp. is constant and change in internal energy is 0. |
| Adiabatic Processes' Constant Variable | Not heat is exchanged. |
| Isobaric Processes' Constant Variable | Pressure is held constant. |
| Isovolumetric (isochoric) Processes | Volume is held constant and work done by or on the system is 0. |
| 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). |
| Entropy | Measure of how much energy has spread out or how spread out energy has become. |
| 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. |
| 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. |
| Farenheit Equation | F = 9/5C + 32, K= C + 273 |
| Thermal Expansion Equation | Del. L = alpha*L*Del.T |
| Volume Expansion Equation | Del. V = Beta*V*DelT |
| First Law of Thermodynamics | Del. U = Q - W |
| Heated Gained Or Lost (With Temperature Change) | q = mcDel.T |
| Heat Gained Or Lost (Phase Change) | q = mL |
| Entropy and Heat | Del. S = Qrev. / T |
| Second Law Of Thermodynamics | Del.S Universe = Del. S System + Del. S Surroundings > 0 |
Created by:
SamB91
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