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Ideal Gases
 

Ideal Gases

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

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

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    Ideal Gases Ideal Gases Presentation Transcript

    • SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY For FULL presentation click HERE >> www.warnescience.net Ideal Gases K Warne
    • 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!!!!
    • 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.
    • 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)
    • 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
    • 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
    • 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)
    • For FULL presentation click HERE >> www.warnescience.net Effect of Temp
    • 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
    • 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.
    • 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
    • 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
    • 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.
    • 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!
    • 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