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CH 13 Gases Review

CH 13 Gases Review. What does STP mean? What the numbers?. Standard Temperature and Pressure 273 K and 1 atm = 760 mm Hg = 760 torr = 101,325 Pa = 101.3 kPa. 2. Explain Boyles law (p, V) Type of relationship (why?) Example?.

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CH 13 Gases Review

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  1. CH 13 Gases Review

  2. What does STP mean? • What the numbers?

  3. Standard Temperature and Pressure • 273 K and 1 atm = 760 mm Hg = 760 torr = 101,325 Pa = 101.3 kPa

  4. 2. Explain Boyles law (p, V) Type of relationship (why?) Example?

  5. Boyles law relates pressure and volume indirectly – as on increases, the other decreases • Ex: crushing a pop can increases pressure so the volume decreases

  6. 3. Explain Charles law –V and T. Type of relationship (why?) Example?

  7. Charles law relates temp and volume directly. As one increases so does the other Ex: hot air balloon (or balloon in lab) as temp increases balloon get bigger (volume inc)

  8. Explain Gay-Lussacs law and give an example

  9. Pressure and temp are directly related • Pressure in tire varies with temp – so in winter when cold, you may need to add more pressure (air) to accommodate for decrease in pressure • Water boils at less than 100°C - syringe and in mountains

  10. What type of relationship is this graph displaying?

  11. Direct • Can you draw the other one?

  12. 4.) 1 mole of any gas at STP has what volume?

  13. 22. 4 L

  14. 5. What is the value and units of the ideal gas constant?

  15. 0.0821 L .atm / moles . K

  16. 6. For a gas, the original pressure is 0.95 atm at 30°C has a volume of 5430 ml. What is the pressure of this gas at 60°C that increased to 6.2 L?

  17. p1V1 = p2 V2 T1 T2 (0.95 atm) (5.43 L) = p2 (6.2 L) 303 K 333 K p2 = 0.914 atm

  18. At 40°C, 7.5 g of ideal oxygen gas occupies 2.5 L. What pressure is exerted on the container?

  19. pV = nRT Need moles 7.5 g O2 1 mole O2 32.0 g O2 0.23 moles O2 pV = nRT p (2.5L) = 0.23 moles (0.0821 mol.K /L.atm) (313K) P = 2.36 atm

  20. A sealed container with flexible walls maintains constant pressure as volume varies with temperature. What is the volume of a gas if a container with 76.5 ml of gas at • -13.0°C is warmed to 125°C?

  21. V/T = V/T • 76.5 ml = V2 • 260K 398 K • V = 117 ml

  22. Frank has a plunger set at 35 ml when the pressure gauge reads 102.1 kPato what volume will the plunger need to be depressed to change the pressure to 30.0 psi?

  23. 102.1 kPa 14.7 psi 101.3 kPa = 14.8 psi pV = pV • (14.8 psi) (35 ml) = (30.0psi) (V) • V = 17.3 ml

  24. What will the volume be at STP of a gas with the original volume of 465 ml at 20.0°C and 98.0kPa?

  25. pV/T = pV/T • (98.0kPa) (465 ml) = (101.3 kPa) (V) 293 K 273K V = 419 ml

  26. Potassium combines with chlorine gas to produce 4.5 g of potassium chloride. How many liters of chlorine gas did it take?

  27. XL 4.5 g 2K + Cl2 2 KCl 4.5 g KCl 1 mole KCl 1 mole Cl2 22.4 L Cl2 74.6 g KCl 2 moles KCl 1 mole Cl2 = 0.68L Cl2

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