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Review for Test 5

This review covers essential gas laws, including Charles's Law, Boyle's Law, Gay-Lussac’s Law, and Dalton’s Law of Partial Pressure. Each law is explained with mathematical relationships and practical examples involving temperature, pressure, and volume calculations. It presents case studies for real-world applications that illustrate how gas behaves under changing conditions and how to determine unknown values using these fundamental principles. Gain insights into the behavior of gases and apply the ideal gas law effectively in various scenarios.

igor-barrera
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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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