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MCAT Gen. Chem Ch. 7
| Term | Definition |
|---|---|
| Isolated Systems | Exchange neither matter nor energy with the environment. |
| Closed Systems | Can exchange energy but not matter with the environment. |
| Open Systems | Can exchange both energy and matter with the environment |
| Isothermal Processes | Occur at a constant temperature. |
| Adiabatic Processes | Exchange no heat with the environment |
| Isobaric Processes | Occur at a constant pressure |
| Isovolumetric (Isochoric) Processes | Processes that occur at a constant volume. |
| State Functions | Describe the physical properties of an equilibrium state. They are pathway independent and include pressure, density, temperature, volume, enthalpy, internal energy, Gibbs free energy, and entropy. |
| Standard Conditions | Defined as 298 K, 1 atm, and 1 M concentrations. |
| Standard State Of An Element Has The Following Standard Conditions: | Standard enthalpy, standard entropy, and standard free energy that is calculated under standard conditions |
| Phase Changes Exist At: | Characteristic temperatures and pressures. |
| Fusion (Melting) And Freezing (Crystallization Or Solidification): | Occur at the boundary between the solid and liquid phases. |
| Vaporization (Evaporation Or Boiling) And Condensation: | Occur at the boundary between the liquid and the gas phases. |
| Sublimation And Deposition: | Occur at the boundary between the solid and gas phases. |
| At Temps Above The Critical Point: | Liquid and gas phases are indistinguishable. |
| At The Triple Point: | All three phases of matter exist in equilibrium. |
| Phase Diagram | Graphs the phases and phase equilibria as a function of temperture and pressure |
| Temperature | Scaled measure of the average kinetic energy of a substance |
| Heat | Transfer of energy that results from differences of temperature between two substances. |
| Enthalpy | Measure of the potential energy of a system found in intermolecular attractions and chemical bonds. This can be calculated using heats of formation, heats of combustion, or bond dissociation energies. |
| Hess's Law | States that the total change in potential energy of a system is equal to the changes of potential energies of the individual steps of the process |
| Entropy | Measure of the degree to which energy has been spread throughout a system or between a system and its surroundings. It is the ratio of heat transferred per mole per unit kelvin. It is maxed at equilibrium. |
| Gibbs Free Energy | Derived from both enthalpy and entropy values for a given system. |
| Delta G < 0 | Reaction proceeds in forward direction (spontaneous) |
| Delta G = 0 | Reaction is in dynamic equilibrium |
| Delta G > 0 | Reaction proceeds in reverse direction (nonspontaneous) |
| Gibbs Free Energy Depends On: | Temperature, specifically temperature-dependent processes change between spontaneous and nonspontaneous |
Created by:
SamB91
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