| A | B |
|---|
| compressibility | Measure of how much the volume of matter decreases under pressure |
| gases | easily compressed |
| space between particles | Gases are easily compressed because of the |
| 10 times the diameter | At room temperature the distance between particles is |
| Kilopascals | Pressure is measured in _______ |
| Liters | Volume is measure in _________ |
| Kelvin | Temperature is measured in ________________ |
| Increases | As more gas is pumped into a rigid closed container the pressure ________ |
| Temperature, pressure and amount of gas | What are some factors that can affect gas pressure |
| Boyles law | If temp. is constant, as the pressure increases, the volume decreases |
| Charles Law | If the pressure is constant, and the temperature increases the volume will increase |
| Gay Lussac | If the volume is constant, and the temp increase so will the pressure |
| Combined gas law | PV/T = PV/T |
| Boyles law | PV = PV |
| Charles Law | V/T = V/T |
| Gay Lussac | P/T = P/T |
| Ideal gas law | PV=nRT |
| low temperatures and high pressures | Real gases differ most from an ideal gas at |
| Daltons law | The total pressure is equal to the partial pressure of the gases |
| partial pressure | Pressure exerted by individual gases in a mixture |
| Diffusion | Tendency of molecules to move to an area of lower concentration |
| effusion | gas escaping through holes in a container |
| Grahams law of effusion | RateA/RateB = sq rt of molar mass B/molar massA |
| Thermochemistry | Study of energy changes that occur during changes |
| chemical potential energy | Energy stored in chemical bonds |
| Heat | q |
| Heat | Energy that transfers from one object to another because of a temp difference |
| Warmer to cooler | Heat always flow from a _____object to a _______ object |
| system | Part of the universe that you are concentrating on |
| surroundings | everything else in the universe |
| Law of conservation of energy | Energy cannot be created nor destroyed |
| endothermic | process that absorbs heat from the surroundings |
| exothermic | Process that gives heat to the surroundings |
| calorie | The amount of heat needed to raise 1 g of pure water 1 deg Celsius |
| Calorie | 1 kilocalorie |
| Calorie | 1000 calories |
| 4.184J | 1 calorie |
| heat capacity | Amount of heat required to raise an object 1 degree Celsius |
| Specific Heat | Amount of heat it takes to raise the temperature 1g of substance 1 deg Celsius |
| enthalpy | H |
| Enthalpy | Heat content in a system |
| Calorimetry | Precise measurement of heat flow |
| Calorimeter | Used to measure absorption or release of heat |
| Heat of reaction | Enthalpy change for the the chemical equation exactly as it is written |
| Heat of fusion | Solid to a liquid |
| Heat of solidification | Liquid to a solid |
| Heat of vaporization | Liquid to a gas |
| Heat of condensation | Gas to a liquid |
| Sublimation | Solid to a gas |
| Exothermic | Delta H is negative |
| Endothermic | Delta H is positive |
