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G - L’s Law – Pressure vs. Temperature

G - L’s Law – Pressure vs. Temperature. Experiment to develop the relationship between the pressure and temperature of a gas. Include : Gay-Lussac’s Law , Combined Gas Law, partial pressure Additional KEY Terms. BOYLE’S LAW – Pressure vs. Volume. P 1 V 1. P 2 V 2. =. Pressure ( kPa ).

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G - L’s Law – Pressure vs. Temperature

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  1. G - L’s Law – Pressure vs. Temperature

  2. Experimentto develop the relationship between the pressure and temperature of a gas. • Include: Gay-Lussac’s Law, Combined Gas Law, partial pressure • Additional KEY Terms

  3. BOYLE’S LAW – Pressure vs. Volume P1V1 • P2V2 = Pressure (kPa) Volume (mL)

  4. CHARLES’S LAW – Temp vs. Volume • T1 • T2 V1 • V2 = Volume (mL) Temperature (K)

  5. Joseph Gay-Lussac (1778-1850) Determined that temperature and pressure of a gas is a direct relationship (volume and amount of gas are held constant)

  6. **As with Charles’ Law, temperature in Kelvin. • T1 • T2 P1 • P2 =

  7. If a 12.0 L sample of gas is found to have a pressure of 101.3 kPa at 0.0°C, calculate the new pressure at 128°C if the volume is held constant. P1 • P2 = • T1 • T2 0.0°C + 273 = 273 K128°C +273 = 401 K • 149 kPa 101.3 • P2 = • (401) • 273

  8. Boyle’s Law: Pressure α ___1___ • volume • Charles’ Law: Volume α temperature • Gay-Lussac’s Law: Pressure α temperature P1 V1 • P2 • V2 = • T1 • T2 combined gas law

  9. If a gas occupies a volume of 25.0 L at 25.0°C and 1.25 atm, calculate the volume at 128°C and 0.750 atm. P1 V1 • P2 • V2 = • T1 • T2 25°C + 273 = 298 K128°C +273 = 401 K (1.25) 25 = • 56.1 L • V2 • (401) • 298 (0.750)

  10. A gas has a volume of 125 L at 325 kPa and 58.0°C, calculate the temperature in Celsius to produce a volume of 22.4 L at 101.3 kPa P1 V1 • P2 • V2 = • T1 • T2 58°C + 273 = 331 K (101.3) • (331) 22.4 • 18.5 K • T2 = • 325 (125) 18.5 K - 273 = -254°C

  11. A bag contains 145 L of air at the bottom of a lake, at a temperature of 5.20°C and a pressure of 6.00 atm. When the bag is released, it ascends to the surface where the pressure is 1.00 atm and 16.0°C. Given: P1 = 6.00 atmV1 = 145LT1 = 5.20°C P2 = 1.00 atmT2 = 16.0°C If the maximum volume of the lift bag is 750 L, will the bag burst at the surface? Find: V2

  12. Dalton’s Law of Partial Pressure: Each gas in a mixture exerts pressure independently. Total pressure = sum of the pressures of each gas (partial pressures) Partial pressure depends on the number of gas particles present, the temperature and volume of container. Ptotal = P1 + P2 + P3 + P4 …

  13. 1.0 mol H2 2.0 mol He 1.0 mol H2 2.0 mol He 3.0 mol gas

  14. The following gases are placed in a 10.00 litre container and held at a constant temperature: 2.0 L of O2 at an original pressure of 202.6 kPa 3.00 L of Ne at an original pressure of 303.9 kPa What pressure is produced inside the container? HINT: Each gas is will expand when put into the 10.00 L container, so each will exert a partial pressure less than its original pressure.

  15. P1V1= P2V2 Oxygen:(202.6)(2.00) = P2 (10.00)P2= 40.5 kPa Neon:(303.9)(3.00) = P2 (10.00)P2= 91.2 kPa Total pressure = 40.5 + 91.2 = 131.7 kPa

  16. CAN YOU / HAVE YOU? • Experimentto develop the relationship between the pressure and temperature of a gas. • Include: Gay-Lussac’s Law, Combined Gas Law, partial pressure • Additional KEY Terms

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