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Chapter 11 KINETIC MOLECULAR THEORY OF AN IDEAL GAS

Chapter 11 KINETIC MOLECULAR THEORY OF AN IDEAL GAS. Particles do not attract or repel Move in straight line Collisions between particles are perfectly elastic G ases come close to ideal behavior at high temperature and low pressure. P pressure

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Chapter 11 KINETIC MOLECULAR THEORY OF AN IDEAL GAS

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  1. Chapter 11KINETIC MOLECULAR THEORYOF AN IDEAL GAS • Particles do not attract or repel • Move in straight line • Collisions between particles are perfectly elastic • Gases come close to ideal behavior at high temperature and low pressure

  2. P pressure • T temperature (must be Kelvin) K = °C + 273) • n moles • V volume

  3. Pressure = Force/Area • More collisions = more pressure • Standard (normal) atmospheric pressure • 760 mm of Hg = 1.00 atm = 101,325 Pa or 101.325 kPa (SI unit) =29.9 inches

  4. P vs V (n and T constant)Boyle’s Law grc.nasa.gov/WWW/K-12/airplane/A...

  5. V vs T (n and P constant)Charles’s Law V T grc.nasa.gov/WWW/K-12/airplane/A...

  6. V vsn (P and T constant)Avogadro’s Law V n grc.nasa.gov/WWW/K-12/airplane/A...

  7. P vsn(V and T constant)Dalton’s Law P moles (n) grc.nasa.gov/WWW/K-12/airplane/A...

  8. P vs T (n and V constant) P T grc.nasa.gov/WWW/K-12/airplane/A...

  9. Combined Gas Law • PV = constant • V/T = constant • P/n = constant • P/T = constant • P1V1/n1T1 = P2V2/n2T2 (when changing a variable) • PV/nT = constant (R) • PV = nRT (Ideal Gas Law) (when looking for one of the 4 variables)

  10. P1V1/n1T1 = P2V2/n2T2 • Ex. If 5.00 liter of gas exert a pressure of 3.0 atm, what pressure will the gas exert if the volume is increased to 10.0 liters? (n and T are constant)

  11. P1V1/n1T1 = P2V2/n2T2 • Ex. If 5.00 liter of gas exert a pressure of 3.0 atm, at a temperature of 25°C what pressure will the gas exert if the volume is increased to 10.0 liters and the temperature is increased to 200°C?

  12. PV=nRT • R = ideal gas constant • R = PV/nT • PV R • atm Liters .0821 atmx L/mol x K • mm Hg Liters 62.4 mmHg x L/mol x K

  13. PV=nRT • Ex. If .10 mole of a gas is added to a 2.0 liter container at a temperature of 25oC, what is the pressure exerted by the gas?

  14. PV=nRT • Ex. What is the molar mass of a gas if .125 grams of the gas occupies .100 L when the temperature is 25oC and the pressure is.728 atm?

  15. PV=nRT • Ex. What is the density of Helium at a pressure of 755 mm Hg and a temperature of 22.0oC?

  16. Standard Temperature and PressureSTP • 0 C ( 273 K) • 1.0 atm ( 760 mmHg) • At STP 1.00 mole of any gas occupies a volume of 22.4 Liters (molar volume)

  17. STP • Ex.If you have 100.0 liter of nitrogen gas at STP, how many moles of nitrogen gas do you have? • Ex.If you have 8.0 mole of carbon dioxide at STP, what volume will it occupy? • Ex. If you have 132 grams of carbon dioxide at STP, what volume will it occupy?

  18. Stoichiometry and Gases • 2H2(g) + O2(g) ---> 2 H2O(g) • Ex.If 5.0 liters of hydrogen gas react, how many liters of oxygen gas are needed? (Gases are at the same temperature and pressure) • Ex.If 3.0 liters of hydrogen gas react, how many liters of water gas are produced? (Gases are at the same temperature and pressure)

  19. Stoichiometry and Gases • 2H2(g) + O2(g) ---> 2 H2O(g) • ex. If 32.0 grams of hydrogen react at STP, what volume of oxygen will be needed? • ex. if 32.0 grams of hydrogen react at a pressure of .500 atm and a temperature of 20.0 oC what volume of oxygen will be needed?

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