Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
10 Gases
Properties of Gases and Gas Laws
| Question | Answer |
|---|---|
| Definition of a gas | A gas is a substance that has no fixed shape or volume and diffuses to fill any container in which it is placed. |
| Temperature used when measuring gases | Kelvin |
| Brownian Motion | Random movement of particles in a gas |
| Pressure of a gas (definition) | The pressure of a gas is the force it exerts per unit area. |
| Units used to measure the pressure of a gas | N/m^2 or the pascal (Pa) |
| Atmospheric pressure in Pascals | 1x10^5 or 100,000Pa or 100kPa |
| Units for measuring the volume of a gas | metres cubed (m3) |
| How to convert cm cubed (cm3) into meters cubed (m3) | divide by 1,000,000 |
| STP | At STP 1 mole of ANY gas will occupy 22.4L |
| Measurements for STP | Standard Temperature: 273K, 0 celcius. Standard Pressure: 1x10^5Pa/100kPa/1atm |
| Boyle's Law | Boyle's Law states that at a constant temperature the volume of a fixed mass of gas is inversely proportional to its pressure. PVB (Increase the pressure, decrease the volume) |
| Relationship between Pressure and 1/Volume | Directly proportional |
| Mathematical conclusion from Boyle's Law | pressure x volume = k |
| Charles Law | Charles' Law states that at a constant pressure the volume of a fixed mass of gas is directly proportional to its temperature on the Kelvin scale (Increase the temperature, Increase the volume) |
| Mathematical conclusion from Charles' Law | Volume/Temperature = k |
| Guy Lussacs' Law of Combining Volumes | Gases react in small whole number ratios provided that their volumes are measured at the same temperature and pressure |
| Avogadro's Law | This states that equal volumes of gases contain equal numbers of molecules, under the same temperature and pressure |
| 4 rules of Kinetic Gas Theory | 1: Particles of a gas are in continuous random motion. 2: There is no attractive or repulsive forces between these molecules 3: There is no difference between the volume of a gas and the container it is in. 4: The collisions are perfectly elastic. |
| Ideal Gas | An ideal gas is a gas that obeys all the assumptions of kinetic theory and all the gas laws at every temperature and pressure. |
| Real Gases behave like Ideal Gases when: | Low pressure as the molecules are far apart. High temperature as the molecules are moving rapidly. |
| Real Gases differ from Ideal gases when: | High pressure as the molecules are pushed close together. Low temperature as they begin to condense into liquids Most gases do exhibit some form of attractive of repulsive forces Collisions are not perfectly elastic |
| Ideal Gas Equation | Pv=nRT |
| Volume of gases in the ideal gas equation | meters cubed |
| Universal Gas Constant | 8.31 J/mol/K |
| Standard volume at room temperature | 24L or 24,000cm3 |
Created by:
Ms O'Farrell
Popular Chemistry sets