Glossary
- Page ID
- 279584
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|---|---|---|---|---|---|
| (Eg. "Genetic, Hereditary, DNA ...") | (Eg. "Relating to genes or heredity") |  |
The infamous double helix | https://bio.libretexts.org/ | CC-BY-SA; Delmar Larsen |
| Word(s) | Definition | Image | Caption | Link | Source |
|---|---|---|---|---|---|
| Adiabatic Process | A thermodynamic process in which no heat is exchanged between a system and its surroundings. | ||||
| Activity | An effective concentration used in non-ideal solutions and gases to account for deviations from ideal behavior. | ||||
| Avogadro’s Law | States that equal volumes of gases at the same temperature and pressure contain an equal number of molecules. | ||||
| Born-Haber Cycle | A thermodynamic cycle used to calculate lattice energy in ionic solids. | ||||
| Buffer | A solution that resists changes in pH when small amounts of acid or base are added. | ||||
| Calorimetry | The measurement of heat flow in chemical reactions and physical changes. | ||||
| Carnot Cycle | A theoretical thermodynamic cycle that describes the most efficient heat engine possible. | ||||
| Chemical Potential | The change in a system’s Gibbs energy with the addition of a mole of a substance, at constant temperature and pressure. | ||||
| Clapeyron Equation | Describes the relationship between pressure, temperature, and phase equilibrium. | ||||
| Colligative Properties | Properties of solutions that depend on solute particle number rather than type, such as boiling point elevation. | ||||
| Degree of Dissociation | The fraction of a dissolved substance that separates into ions in solution. | ||||
| Electrochemical Cell | A system that generates electrical energy from chemical reactions. | ||||
| Entropy | A measure of disorder or randomness in a system. | ||||
| Enthalpy | The heat content of a system at constant pressure. | ||||
| Equation of State | A mathematical equation that describes the state of matter under given conditions, such as the ideal gas law. | ||||
| Fugacity | A corrected pressure term used to describe real gas behavior. | ||||
| Free Energy, Gibbs Free Energy | A thermodynamic quantity used to predict whether a reaction is spontaneous at constant pressure and temperature. | ||||
| Gibbs-Duhem Equation | Relates the chemical potentials of components in a mixture. | ||||
| Graham’s Law of Effusion | States that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. | ||||
| Half-Life | The time required for half of a reactant to be consumed in a reaction. | ||||
| Helmholtz Energy | A thermodynamic function that measures the work potential of a system at constant volume and temperature. | ||||
| Ideal Gas Law | An equation describing the state of an ideal gas: PV=nRT. | ||||
| Joule-Thomson Effect | Describes the temperature change of a real gas when it is expanded or compressed without heat exchange. | ||||
| Kinetic Molecular Theory | A model that explains gas behavior based on particle motion and collisions. | ||||
| Lattice Energy | The energy required to separate an ionic solid into its gaseous ions. | ||||
| Le Chatelier’s Principle | States that a system at equilibrium will adjust to counteract applied changes. | ||||
| Maxwell’s Relations | A set of thermodynamic equations derived from the symmetry of second derivatives of thermodynamic potentials. | ||||
| Michaelis-Menten Mechanism | A model describing enzyme-catalyzed reactions. | ||||
| Non-Ideal Solution | A solution that deviates from Raoult’s law due to intermolecular interactions. | ||||
| Partial Molar Volume | The volume contribution of a component in a mixture. | ||||
| Phase Diagram | A graphical representation of phase stability as a function of temperature and pressure. | ||||
| Pressure Dependence of Gibbs Energy | Describes how Gibbs energy varies with pressure. | ||||
| Raoult’s Law | States that the vapor pressure of a solvent is proportional to its mole fraction in solution. | ||||
| Reaction Mechanism | A step-by-step description of how a chemical reaction occurs. | ||||
| Reaction Rate | The speed at which reactants are converted to products. | ||||
| Solubility | The ability of a substance to dissolve in a solvent. | ||||
| Standard Reduction Potential | A measure of the tendency of a chemical species to gain electrons. | ||||
| Steady-State Approximation | Assumes that the concentration of reaction intermediates remains constant over time. | ||||
| Temperature Dependence of Equilibrium Constant | Describes how equilibrium constants change with temperature. | ||||
| Transition State Theory | A model describing the high-energy transition state of a reaction. | ||||
| Van ’t Hoff Equation | Relates temperature changes to equilibrium constant changes. | ||||
| Volume Dependence of Helmholtz Energy | Explains how Helmholtz energy changes with volume variations. |