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Ideal Gases
K Warne
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Gas Problems – Aerosol cans
Q...
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Gas Problems
• Explain how an...
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Gas Problems
1. If a car tyre...
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Temperature Scales
• 0° Celsi...
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Macroscopic / microscopic
Kin...
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Effect of Temperature - Guy L...
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Effect of Temp
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A weather balloon has a volum...
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Pressure & Volume
If the ____...
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Boyles Law
Spreadsheet
T = 29...
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Ideal Gas Deviations
Real gas...
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Ideal Gas Deviations
At low _...
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Real Gases - Deviations
Real ...
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Ideal Gases

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Powerpoint to teach ideal gases and deviations from ideal gas behaviour to high school students

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Ideal Gases

  1. 1. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Ideal Gases K Warne
  2. 2. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Gas Problems – Aerosol cans Question: Pressurized containers (aerosol cans) carry warnings to avoid heating the container. Why is this? Describe a gas law that relates to this problem and explain it’s relevance in terms of the Kinetic Theory of Gases. NO!!!!
  3. 3. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Gas Problems • Explain how and why real gases differ from the behaviour of an ‘ideal gas’. Real gases deviate from the ideal gas model - this occurs at high pressure and low temperature. 1. At high pressure • the particles are forced close together and their volume adds to the total volume of the gas. • The volume of the real gas is larger than that of an ideal gas at high pressure. 2. At low temperature • the forces between the particles pull them closer together. • The volume of the real gas is therefore lower than that of an ideal gas.
  4. 4. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Gas Problems 1. If a car tyre has a pressure of 280 kPa at 25o C, what would the pressure be if the tyre temperature heats up to 38o C on a long journey? (Assuming the volume stays constant.) P1 = P2  T1 T2 280000 = P2  298 311 P2 = 260906 Pa  = 292.21 kPa (4)
  5. 5. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Temperature Scales • 0° Celsius = 273Kelvin • ABSOLUTE ZERO 0 Kelvin = -273°C • Celsius Kelvin …………………… • Kelvin Celsius ……………………. Convert to K: Boiling point water 100o C Room Temp 25o C Body Temperature 37o Kelvin Celsius Fahrenheit
  6. 6. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Macroscopic / microscopic Kinetic theory relates the ________________ properties of substances to its ___________________ properties. Pressure= force/area Volume =lxb h Temperature = o C or K Pressure: _________________ per unit _________. Temperature: is a measure of the _____________________ of particles. Macroscopic properties: ___________, ___________, ____________ Microscopic properties: ________ & ________ of particles
  7. 7. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Effect of Temperature - Guy Lussacs’ Law The temperature of a fixed mass of gas is increased while the volume is kept constant. Guy Lussack's Law P (Pa) x103 T (K) V = const 100 298.0 x1.4 120 357.6 x 1.4 140 417.2 160 476.8 180 536.4 x 2 200 596.0 x 2 The temperature is directly proportional to the pressure - if the pressure doubles the temperature would also double. 0.0 100.0 200.0 300.0 400.0 500.0 600.0 700.0 0 50 100 150 200 250Temperature(K) Pressure (Pa) x 103 T (K)
  8. 8. For FULL presentation click HERE >> www.warnescience.net Effect of Temp
  9. 9. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net A weather balloon has a volume of 5 dm3 at sea level when the temperature is 25o C. What would the volume of the balloon be if the temperature rose to 35o C on a hot day? Pressure - volume example. Given: V1 = 5 dm3 T1 = 25 + 273 = 298 K T2 = 35 + 273 = 308K Asked: V2 V1/ T1 = V2 /T2 (5/298) = V2 / 308 V2 = 308*(5/298) = 5.17 dm3
  10. 10. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Pressure & Volume If the __________ of a fixed mass of gas is _______ the _________ will increase. (T = const.) The pressure increases because… This happens because there is ________ for the particles to collide with so the ______ of __________ with the sides of the container _____________ increases.
  11. 11. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Boyles Law Spreadsheet T = 298K Volume vs Pressure for a fixed mass of gas (T = const) 10 15 20 25 30 35 40 45 50 55 55 75 95 115 135 155 175 195 215 Boyle's Law Pressur e (kPa) Volume (cm3) 200 15 150 17 118 21 96 27 80 35 69 42 P  1/V P = k (1/V) pV = k
  12. 12. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Ideal Gas Deviations Real gases deviate from the ideal gas model - this occurs at __________________ and ___________________. At high ___________________ • the particles are _____________ and their _____________ adds to the ____________ of the gas. • The volume of the real gas is ______________ than that of an ideal gas at high pressure. P
  13. 13. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Ideal Gas Deviations At low ______________ • the _____________ between the particles pull them ___________ together. • The volume of the real gas is therefore __________ than that of an ideal gas.
  14. 14. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Real Gases - Deviations Real gases deviate from ideal behavior at low __________ and high ____________. Many real gases ___________ under these conditions. At low __ and low ___ Real gas particles are _______ ______ by attractive forces - they therefore exert _____ ___________. Indicate these areas on the graph!
  15. 15. SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Hi - This is a SAMPLE presentation only. My FULL presentations, which contain a lot more more slides and other resources, are freely available on my resource sharing website: www.warnescience.net (click on link or logo) Have a look and enjoy! WarneScience
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