Term
|
Definition
| device designed to measure the energy change for processes occurring under conditions of constant volume; commonly used for reactions involving solid and gaseous reactants or products |
|
|
Term
|
Definition
| (also, bond dissociation energy) energy required to break a covalent bond in a gaseous substance |
|
|
Term
|
Definition
| thermochemical cycle relating the various energetic steps involved in the formation of an ionic solid from the relevant elements |
|
|
Term
|
Definition
| unit of heat or other energy; the amount of energy required to raise 1 gram of water by 1 degree Celsius; 1 cal is defined as 4.184 J |
|
|
Term
|
Definition
| device used to measure the amount of heat absorbed or released in a chemical or physical process |
|
|
Term
|
Definition
| process of measuring the amount of heat involved in a chemical or physical process |
|
|
Term
|
Definition
| area of science that deals with the relationships between heat, work, and all forms of energy associated with chemical and physical processes |
|
|
Term
|
Definition
| chemical reaction or physical change that absorbs heat |
|
|
Term
|
Definition
| capacity to supply heat or do work |
|
|
Term
|
Definition
|
|
Term
|
Definition
| heat released or absorbed by a system under constant pressure during a chemical or physical process |
|
|
Term
|
Definition
| chemical reaction or physical change that releases heat |
|
|
Term
| expansion work (pressure-volume work) |
|
Definition
| work done as a system expands or contracts against external pressure |
|
|
Term
| first law of thermodynamics |
|
Definition
| internal energy of a system changes due to heat flow in or out of the system or work done on or by the system |
|
|
Term
|
Definition
| transfer of thermal energy between two bodies |
|
|
Term
|
Definition
| extensive property of a body of matter that represents the quantity of heat required to increase its temperature by 1 degree Celsius (or 1 kelvin) |
|
|
Term
|
Definition
| if a process can be represented as the sum of several steps, the enthalpy change of the process equals the sum of the enthalpy changes of the steps |
|
|
Term
|
Definition
| compound composed only of hydrogen and carbon; the major component of fossil fuels |
|
|
Term
|
Definition
| total of all possible kinds of energy present in a substance or substances |
|
|
Term
|
Definition
| SI unit of energy; 1 joule is the kinetic energy of an object with a mass of 2 kilograms moving with a velocity of 1 meter per second, 1 J = 1 kg m2/s and 4.184 J = 1 cal |
|
|
Term
|
Definition
| energy of a moving body, in joules, equal to |
|
|
Term
| lattice energy (?Hlattice) |
|
Definition
| energy required to separate one mole of an ionic solid into its component gaseous ions |
|
|
Term
| nutritional calorie (Calorie) |
|
Definition
| unit used for quantifying energy provided by digestion of foods, defined as 1000 cal or 1 kcal |
|
|
Term
|
Definition
| energy of a particle or system of particles derived from relative position, composition, or condition |
|
|
Term
| specific heat capacity (c) |
|
Definition
| intensive property of a substance that represents the quantity of heat required to raise the temperature of 1 gram of the substance by 1 degree Celsius (or 1 kelvin) |
|
|
Term
| standard enthalpy of combustion |
|
Definition
| heat released when one mole of a compound undergoes complete combustion under standard conditions |
|
|
Term
| standard enthalpy of formation |
|
Definition
| enthalpy change of a chemical reaction in which 1 mole of a pure substance is formed from its elements in their most stable states under standard state conditions |
|
|
Term
|
Definition
| set of physical conditions as accepted as common reference conditions for reporting thermodynamic properties; 1 bar of pressure, and solutions at 1 molar concentrations, usually at a temperature of 298.15 K |
|
|
Term
|
Definition
| property depending only on the state of a system, and not the path taken to reach that state |
|
|
Term
|
Definition
| all matter other than the system being studied |
|
|
Term
|
Definition
| portion of matter undergoing a chemical or physical change being studied |
|
|
Term
|
Definition
| intensive property of matter that is a quantitative measure of |
|
|
Term
|
Definition
| kinetic energy associated with the random motion of atoms and molecules |
|
|
Term
|
Definition
| study of measuring the amount of heat absorbed or released during a chemical reaction or a physical change |
|
|
Term
|
Definition
| energy transfer due to changes in external, macroscopic variables such as pressure and volume; or causing matter to move against an opposing force |
|
|
