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Unit 5 Vocabulary
Term | Definition |
---|---|
Phase Diagram | A graph of pressure and temperature that shows the conditions under which a substance exists. |
STP | Standard Temperature and Pressure |
Triple Point | The temperature and pressure at which the solid, liquid, and gas phases co-exists. |
Critical Point | Where substance indicates the critical temperature and critical pressure. |
Molar Enthalpy of Fusion | The amount of energy required to melt one mole of a solid |
Nonvolatile | Liquids that do not evaporate readily because of strong attractive forces between particles. |
Deposition | The change of a gas directly to a solid. |
Sublimation | The change of a solid directly to a gas |
Kinetic molecular theory | Particles are in constant motion |
Molar Enthalpy of Vaporization | The amount of energy as heat needed to vaporize one mole of a liquid. |
∆H | enthalpy of products - enthalpy of reactants |
Hess' Law | Overall enthalpy change in a reaction is equal to the sum of the enthalpy changes for the individual steps in the process. |
Endothermic | Heat energy is absorbed; products higher |
Exothermic | Heat energy released; products lower |
Enthalpy Change | using Hess' law; process equals the sum of the energy difference of products minus the sum of the energy difference of the reactants |
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