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Pressure

Pressure. Pressure is:. “Amount of force per unit area”. Force =. Pressure. Pressure depends on two things:. 1 ). 2 ). Pressure. Units of standard pressure:. atmosphere :. millimeters of mercury :. torr :. kilopascal :. Increases and Decreases in Pressure. Effect of temperature.

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Pressure

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  1. Pressure Pressure is: “Amount of force per unit area” Force =

  2. Pressure Pressure depends on two things: 1) 2)

  3. Pressure Units of standard pressure: atmosphere: millimeters of mercury: torr: kilopascal:

  4. Increases and Decreases in Pressure Effect of temperature Temperature goes up, Temperature goes down, Temperature and pressure are ____________ related

  5. Increases and Decreases in Pressure Effect of volume Volume goes up, Volume goes down, Volume and pressure are _____________ related

  6. Increases and Decreases in Pressure Effect of number of particles # of particles goes up, # of particles goes down, # of particles and pressure are ____________ related

  7. “Laws” Boyle’s Law – Volume and pressure are inversely related assumes _________________________ are constant

  8. “Laws” Charles’s Law – Temperature and volume are directly proportional ______________________ ______________________ assumes _________________________are constant

  9. “Laws” Gay-Lussac’s Law – Temperature and pressure are directly proportional ______________________ ______________________ assumes _______________________ are constant

  10. “Laws” Avogadro’s Law – Particles and Volume Particles and volume are directly proportional assumes _______________________ are constant

  11. Molar Volume molar means “_____________” molar volume means ____________________ molar volume means ________________________

  12. GASES • All gases at the same temperature have the same molar volume (all at 1 atm) He CO2 1 mol @ 0 oC 1 mol @ 100 oC 1 mol @ 1000 oC

  13. Molar Volume 1 mol of ______ gas = _______ of gas @ _____ STP = __________________and ________ __________ _______

  14. Avogadro’s # The mole Only 2 options of what to do with the mole: mole particles molar mass mole mass mole-to-mole ratio mole “X” mole “Y”

  15. mol RECAP 1 molH2(g)= ___________________ H2(g) 1 mol H2(g) = _______ H2(g) 1 mol H2(g) = ______ L H2(g) (@ _____)

  16. more mol calculations What mass of chlorine gas occupies 13.90 L at STP?

  17. “Laws” Combined Gas Law – Combination of Boyle’s, Charles’s, and Gay-Lussac’s assumes ______________is constant

  18. “ “Laws” ” “Super Combined Gas Law” – Pressure, Temperature, Particles, and Volume Combination of Boyle’s, Charles’s, Avogadro’s, and Gay-Lussac’s

  19. “ “Laws” ” You need to know how these variables are related P V P T P n T n V T V n

  20. Using Ratios __1, so the answer is __________ than 6 __1, so the answer is __________ than 6 Larger number on ________________ __________ answer (number goes ________) Larger number on ________________ __________ answer (number goes ________)

  21. Using Ratios __1, so the answer is ________ than 31 __1, so the answer is ________ than 31 Larger number on ________________ __________ answer (number goes ________) Larger number on ________________ __________ answer (number goes ________)

  22. Did you get it? A steel container filled with nitrous oxide at 15.0 atm is cooled from 25.0 ºC to -40.0ºC. Calculate the final pressure.

  23. Dalton’s law of partial pressures states that the total pressure of a gaseous mixture is equal to the sum of the individual pressures of each gas. • The pressure exerted by each gas in a mixture is its ________________________, Pn.

  24. An atmospheric sample contains nitrogen, oxygen, argon, and traces of other gases. If the partial pressure of nitrogen is 587 mmHg, oxygen is 158 mmHg, and argon is 7 mmHg, what is the observed pressure as read on the barometer?

  25. We can measure the volume of a gas by displacement. • By collecting the gas in a graduated cylinder, we can measure the amount of gas produced. • The gas collected is referred to as “wet” gas since it also contains water vapor.

  26. 672.43 mL of hydrogen was collected over water on a day when the barometer read 661.2 mmHg. The temperature of the wet gas was 25 oC. 1) What is the partial pressure of the gas? (vapor pressure of water at 25 oC is 23.8 mmHg)

  27. 672.43 mL of hydrogen was collected over water on a day when the barometer read 661.2 mmHg. The temperature of the wet gas was 25 oC. 2) What is the volume of the gas at STP?

  28. 672.43 mL of hydrogen was collected over water on a day when the barometer read 661.2 mmHg. The temperature of the wet gas was 25 oC. 3) What was the mass of hydrogen collected?

  29. Ideal Gas Law • An ideal gas is a gas that behaves in a predictable and consistent manner. • Ideal gases have the following properties:

  30. Ideal Gas Law

  31. Ideal Gas Law What is the temperature of 0.250 mol of chlorine gas at 655 torr if the volume is 3.50 L?

  32. Ideal Gas Law How many grams of NO2 gas occupy a volume of 0.8635 L at 0.9446 atm and 25 oC?

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