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Chem Unit 5 Vocab

TermDefinition
Triple Point the temperature and pressure at which the solid, liquid, and vapor phases of a pure substance can coexist in equilibrium.
Kinetic molecular theory the model describes a gas as a large number of identical submicroscopic particles, all of which are in constant, rapid, random motion.
STP standard temperature and pressure are standard sets of conditions for experimental measurements to be established to allow comparisons to be made between different sets of data.
Critical Point in thermodynamics, a critical point is the end point of a phase equilibrium curve.
Molar enthalpy of fusion the amount of energy needed to change one mole of a substance from the solid phase to the liquid phase at constant temperature and pressure.
Deposition deposition occurs when molecules settle out of a solution.
Phase Diagram is a graphical representation of the physical states of a substance under different conditions of temperature and pressure.
Exothermic (of a reaction or process) accompanied by the release of heat.
△ H that means the reaction is exothermic
Enthalpy change the standard enthalpy of reaction is the enthalpy change that occurs in a system when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.
Nonvolatile refers to a substance that does not readily evaporate into gas under existing conditions.
Hess' Law regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes.
Endothermic (of a reaction or process) accompanied by or requiring the absorption of heat.
Molar Mass of Vaporization if the substance in question is a volatile liquid, a common method to determine its molar mass is to vaporize it and apply the ideal gas law, PV = nRT to the data collected.
Sublimation the conversion between the solid and the gaseous phases of matter, with no intermediate liquid stage.
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