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Review for Test 5

Review for Test 5. Gas Laws. Charles Law V 1 = V 2 P constant T 1 T 2 Boyles Law P 1 V 1 = P 2 V 2 T constant Gay-Lussac’s Law P 1 = P 2 V constant T 1 T 2 Combined P 1 V 1 = P 2 V 2

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Review for Test 5

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  1. Review for Test 5 Gas Laws

  2. Charles LawV1 =V2 P constant T1 T2 Boyles Law P1V1 = P2V2 T constant Gay-Lussac’s Law P1=P2 V constant T1 T2 CombinedP1V1=P2V2 T1 T2 Ideal Gas Law PV = nRT

  3. Dalton’s Law of Partial Pressure The sum of the individual gas pressures equals the overall pressure of the mixture of gases. P1 + P2 + P3 . . . = Ptotal

  4. A sample of gas occupies 2.97 L at 72˚C. What volume would it take up at 502K? V1 =V2 T1 T2 Volume should increase! 2.97L x 502K = 4.32 L 345K

  5. A gas-filled bottle is heated from 25°C to 89°C. If the original pressure was 760 torr, what would be the new pressure ? T1 = 25+273=298K T2 = 89+273=362K 760 = P2 298 362 P2 = 923 torr

  6. A gas at 98.2 kPa has a volume of 39L. What is its volume at 120.5kPa and constant temperature? P1V1 = P2V2 Volume should decrease. 39L x 98.2 kPa = 31.8L 120.5 kPa

  7. At STP, the volume of a gas is 325 mL. What volume does it occupy at 20.0°C and 93.3kPa? P1V1=P2V2 T1 T2 325 mL x 293K x 101.3 kPa = 379 mL 273K 93.3 kPa

  8. What pressure is exerted by .00306 mole of gas in a 25.9 cm3 container at 9˚C? P= nRT V = .00306mol x 8.31 L∙kPa x 282K .0259 L mol∙K = 277kPa

  9. A 35.0L tank contains 7.00 mol of compressed air. If the pressure inside the tank is 500.0 kPa, what is the temperature of the compressed gas? T = PV nR T = 500.0kPa x 35.0L 7.00mol x 8.31 = 301 K

  10. A gaseous mixture containing argon, nitrogen, and oxygen is in a vessel. If the total pressure is 98.5 kPa, and the partial pressures of nitrogen and argon are 22.0 kPa and 50.0 kPa respectively, what is the partial pressure of oxygen? Ptot = PAr + PN + PO 98.5 kPa = 22.0 + 50.0 + Po PO = 26.5 kPa

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