Kinetic Theory, Reaction Rates and Energy Effects
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Created by:
jannika12 on May 22, 2012
Subjects:
Description:
quantitive relationships between gases, colligative properties, vapour pressure and boiling pressure, and energy effects.
Classes:
Kinetic Theory, Equilibrium, Reactions, Energy Effects and Rates
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8 terms
Terms | Definitions |
|---|---|
 Boyle's Law (P+V): | Pressure and volume are INVERSELY proportional. i.e. -as pressure increase, volume decreases. -as pressure decreases, volume increases. P1V1 = P2V2 |
| Charle's Law (V+T): | Volume and temp. are DIRECTLY proportional i.e if temp increases, volume increases & if temp decreases, volume decreases. V1/T1 = V2/T2 *Use KELVIN (K) rather than celsius. ^0C + 273 = K K - 273 = ^0C |
| Combined Gas Law (P,V and T): | P1V1/ T1 = P2V2/T2 |
| Colligative Properties: | Vapour pressure, melting temperature and boiling temperature. *Applies to liquids and solutions. |
| Boiling Pressure: | As a liquid boils, bubbles of gas form inside the liquid, and if there's enough pressure inside the bubble, it will rise to the surface, burst and release vapour. => When MAX vapour pressure = Atmosphere Pressure |
| Define: Vapour Pressure | Collisions of the vapour from the liquid. |
| Adding a Solute (Effects on Boiling Point and Melting Point): | B.Point and M.Point are changed by adding another chemical; B.point increases, but freezing point decreases. The more moles of solute (i.e. greater number of particles attracting H2O), the higher the boiling point (due to increased number of ions). |
| Energy Effects: | -Energy is measured in kJ, and in an equations, kJ/mol. -Reactants have a given amount of chemical energy/ enthalpy (Hr). - Products have a given amount of enthalpy (Hp). => The amount of energy GIVEN OUT OR ABSORBED is called the HEAT OF THE REACTION. |
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