1. Gases

2. Properties: Gases are fluids because their molecules/atoms can flow Gases have low density - atoms are far apart from each other Highly compressible – their volume can be reduced Gases will completely fill their container

3. Gas Pressure PRESSURE is a force exerted by the substance per unit area on another substance. GAS PRESSURE is the force that the gas exerts on the walls of its container. A balloon expands because the pressure of the gas molecules inside is greater than the pressure of the gas molecules on the outside. http://www.indiana.edu/~geog109/topics/10_Forces&Winds/GasPressWeb/PressGasLaws.html

4. Gas Pressure http://www.indiana.edu/~geog109/topics/10_Forces&Winds/GasPressWeb/PressGasLaws.html Gas (air) on the outside of the balloon is exerting pressure onto surface of the balloon. The atmospheric pressure outside a balloon, P A, is the impact of moving gas molecules as they collide with the skin of the balloon.

5. Atmospheric Pressure If you could measure the weight of a column of air above the surface of the Earth, it would be14.70 lbs per square inch! This is also known as 1 atmosphere or 1 atm

6. Atmospheric Pressure As you descend toward earth, the atmosphere is denser and the pressure is higher When flying your ears may “Pop” due to the change in pressure

7. Pressure Conversions There are many units to express pressure: - pounds per square inch (tire pressure) - atmospheres - torr - pascals - mm of Hg - bars We need to be able to convert between units.

8. Converting between units Use dimensional analysis! Ex: Convert the pressure of 1.000 atm to mm of mercury Conversion factor: 101325 Pa and 1 mm Hg 1 atm 133.322 Pa Calculation: 1.000 atm x 101325 Pa x 1 mm Hg = 760 mm Hg 1 atm 133.322 Pa

9. Gases – Converting Between Units UnitAbbreviationConversion Factor Atmosphereatm1 atm = 101.325 kPa Millimeters of HgmmHg760 mm Hg = 1 atm Torrtorr760 torr = 1 atm PascalPa101.325 kPa = 101325 Pa Millibarbar1013.2 millibar = 1 atm

10. Pressure Conversions Practice The pressure of carbon dioxide is 72.7 atm. What is this value in units of kilopascals? The pressure of water vapor at 50 deg C is 12.33kPa. What is this value in mm of Hg?

11. Variables in Gas Laws Whenever we discuss gas laws, we are interested in 4 variables: Number of moles of gas Volume of gas Pressure of gas Temperature of gas

12. First Gas Law: Boyle’s Law Pressure-Volume Relationships Boyle’s Law Based on the following facts: 1. Gases can be compressed 2. Gases exert pressure Boyle found that: As volume decreases, the concentration, and therefore the pressure, increases

13. Boyle’s As volume decreases, the concentration, and therefore the pressure, increases

14. Gases Boyle’s Law States: For a fixed amount of gas at a constant temperature: as the volume of the gas decreases the pressure increases We can use the following equation to calculate changes in pressure or volume

15. Boyle’s Law A graph of Boyle’s Law shows the relationship between pressure and volume is inversely proportional: as one variable increases, the other decreases

16. Boyle’s Law http://www.grc.nasa.gov/WWW/K- 12/airplane/aboyle.html Animation of Boyle’s Law

17. Boyle’s Law Example: A given sample of gas occupies 523 mL at 760 torr. The pressure is increased to 1.97 atm, while the temperature remains the same. What is the new volume of gas?

18. Second Gas Law: Charles’ Law Temperature-Volume Relationships Charles’ Law For a fixed amount of gas at a constant pressure, the volume of a gas increases as the temperature of the gas increases

20. Charles’ Law Graph The graph of Charles’ Law is a straight line (linear). It shows the relationship between temperature and volume is directly proportional: as one variable increases or decreases, so does the other

21. Charles’ Law Formula: Remember! ALWAYS USE KELVIN when dealing with temperature in gas laws! All °C temperatures MUST be converted to Kelvin!!!

22. Charles’ Law http://wright.nasa.gov/airplane/aglussac.html Animation of Charles’ Law

23. Charles’ Law Example: A balloon is inflated to 665 mL volume at 27 deg C. It is immersed in a dry-ice bath at -78.5 deg C. What is its new volume, assuming the pressure remains constant?

24. Third Gas Law: Gay-Lussac’s Law Temperature-Pressure Relationships Gay-Lussac’s Law: The pressure of a gas at a constant volume is directly proportional to the absolute temperature (temperature in Kelvin)

25. Gay-Lussac’s Animation http://www.chm.davidson.edu/ChemistryAppl ets/KineticMolecularTheory/PT.html http://www.chm.davidson.edu/ChemistryAppl ets/KineticMolecularTheory/PT.html

26. Gay-Lussac’s Law Formula: At constant volume: P 1 = P 2 T 1 T 2

27. Avogadro’s Law In 1811, Avogadro proposed that equal volumes of all gases, under the same conditions, have the same number of particles.

28. Avogadro’s Law We know volume of a gas can change with temperature and pressure, but what about the number of molecules? Through Avogadro’s observations, the following has been defined: 1 mole of any gas at STP (0°C and 1 atm) occupies 22.41 L The mass of 22.41L at STP is the Molecular Mass of the gas

29. Combined Gas Law When you take Boyles, Charles’, Gay- Lussac’s and Avogadro’s Laws and combine them, you get the COMBINED GAS LAW This law is used to solve problems where pressure, volume and temperature of a gas vary with a constant molar quantity of the gas

30. Combined Gas Law Example: A sample of hydrogen gas has a volume of 65.0 mL at a pressure of 0.992 atm and a temperature of 16 deg C. What volume will be hydrogen occupy at 0.984 atm and 25 deg C?

31. Dalton’s Law of Partial Pressures John Dalton showed that in a mixture of gases, each gas exerts a certain pressure as if it were alone with no other gases with it. This is called “partial pressure” Equation: P t = P 1 + P 2 + P 3 …………

32. Dalton’s Law of Partial Pressures

33. Example: A 2.5 L flask at 15 deg C contains a mixture of three gases: N 2, He, and Ne. The partial pressures are: N 2 = 0.32 atm, He = 0.15 atm and 0.42 atm for Ne. What is the total pressure of the system?

34. Gases – Dalton’s Law of Partial Pressures – Mole Fraction As Dalton’s Law tells us, if a number of gases are mixed, each contributes to the pressure in its vessel. To figure out how much pressure one gas is contributing, we need to find: 1. Mole Fraction 2. Its partial pressure.

35. Gases – Mole Fraction/Partial Pressure To calculate mole fraction (X): X ? = moles of gas of interest total moles of gas in the mixture To calculate the partial pressure of that gas: P x = X ? P total

36. Gases – Mole Fraction/Partial Pressure A mixture of gases contains 4.46 moles of neon (Ne), 0.74 moles of argon (Ar) and 2.15 moles of xenon (Xe). Calculate the partial pressure of Ne.

37. Gas Simulator http://intro.chem.okstate.edu/1314F00/Labor atory/GLP.htm http://intro.chem.okstate.edu/1314F00/Labor atory/GLP.htm