| Term | Definition |
|---|
| Brønsted-Lowry base | a substance that accepts a proton |
| calorimeter | a device used to measure the heat absorbed or released in a chemical or physical change |
| enthalpy change | the amount of energy absorbed or released as heat by a system during a process at constant pressure |
| enthalpy of combustion | enthalpy of combustion |
| enthalpy of reaction | the amount of energy released or absorbed as heat during a chemical reaction |
| entropy | a measure of the randomness or disorder of a system |
| free energy | the energy in a system that is available for work; a system's capacity to do useful work |
| heat | the energy transferred between objects that are at different temperatures |
| Hess's law | the overall enthalpy change in a reaction is equal to the sum of the enthalpy changes for the individual steps in the process |
| joule | the unit used to express energy; equivalent to the amount of work done by a force of 1 N acting through a distance of 1 m in the direction of the force (abbreviation, J) |
| molar enthalpy of formation | the amount of energy as heat resulting from the formation of 1 mol of a substance at constant pressure |
| specific heat | the quantity of heat required to raise a unit mass of homogeneous material 1 K or 1°C in a specified way given constant pressure and volume |
| temperature | a measure of how hot (or cold) something is; specifically, a measure of the average kinetic energy of the particles in an object |
| thermochemical equation | an equation that includes the quantity of heat released or absorbed during the reaction as written |
| thermochemistry | the branch of chemistry that is the study of the heat changes that accompany chemical reactions and changes of state |
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