Properties of Gases and Gas Laws
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| 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.
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| Temperature used when measuring gases | Kelvin
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| Brownian Motion | Random movement of particles in a gas
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| Pressure of a gas (definition) | The pressure of a gas is the force it exerts per unit area.
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| Units used to measure the pressure of a gas | N/m>2 or the pascal
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| Atmospheric pressure in Pascals | 1x10>5 or 100,000Pa or 100kPa
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| Units for measuring the volume of a gas | metres cubed
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| How to convert cm cubed into meters cubed | divide by 1,000,000
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| STP | At STP 1 mole of ANY gas will occupy 22.4L
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| Measurements for STP | Standard Temperature: 273K, 0 celcius.
Standard Pressure: 1x10>5Pa/100kPa/1atm
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| 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.
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| Relationship between Pressure and 1/Volume | Directly proportional
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| Mathematical conclusion from Boyle's Law | pressure x volume = k
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| 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
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| Mathematical conclusion from Charles' Law | Volume/Temperature = k
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| 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
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| Avogadro's Law | This states that equal volumes of gases contain equal numbers of molecules, under the same temperature and pressure
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| 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.
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| 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.
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| Real Gases behave like Ideal Gases when: | Low pressure as the molecules are far apart.
High temperature as the molecules are moving rapidly.
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| 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
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| Ideal Gas Equation | Pv=nRT
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| Volume of gases in the ideal gas equation | meters cubed
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| Universal Gas Constant | 8.31
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