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The Erlenmeyer

The Erlenmeyer . What happens when a piece of paper is placed overtop of a rigid container filled with water and the container is inverted? Calculate the amount of force being applied by the atmosphere on the piece of paper. What volume of water would be required to move the paper?.

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The Erlenmeyer

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  1. The Erlenmeyer • What happens when a piece of paper is placed overtop of a rigid container filled with water and the container is inverted? • Calculate the amount of force being applied by the atmosphere on the piece of paper. • What volume of water would be required to move the paper?

  2. The Empirical Gas Laws Unit 5 Chapter 11

  3. Boyle’s Law • Published in 1662 by Robert Boyle, it states that for a fixed amount of a gas at a fixed temperature, the pressure of the gas is inversely proportional to the volume of the gas. • P ∝ V-1 • Generalizing this, we get • P1V1 = P2V2

  4. Boyle-ing your Brain • A gas occupies 17.4 liters at 0.862 atm. What is the pressure if the volume becomes 15.0 L?

  5. Charles’s Law • Published in 1802 by Joseph Gay-Lussac based off of work from the 1780’s by Jacques Charles, it states that for a fixed amount of a gas at a fixed pressure, the volume of the gas is directly proportional to the temperature of the gas. • V ∝ T • Generalizing this, we get (since there is a sign inversion at 0 °C, always use Kelvin) • V1/T1 = V2/T2

  6. Giving Your Brain a Charlie Horse • The temperature of a 4.00 L sample of gas is changed from 10.0 °C to 20.0 °C. What will the volume of this gas be at the new temperature?

  7. Pressure/Temperature Law • Published in 1702 by Guillaume Amontons but made famous by Gay-Lussac (in the same paper from 1802), it states that for a fixed amount of a gas at a fixed volume, the pressure of the gas is directly proportional to the temperature of the gas. • P ∝ T • Generalizing this, we get (remember to always use Kelvin) • P1/T1 = P2/T2

  8. Feeling the Pressure • If a gas in a closed container is pressurized from 15.0 atm to 16.5 atm and its original temperature was 23.7 °C, what would the final temperature of the gas be?

  9. The Combined Gas Law • Combining Boyle’s, Charles’s, and the Pressure/Temperature Law, assuming a fixed amount of gas, we get: • (Always use Kelvin!) • P1V1/T1 = P2V2/T2

  10. I’ll Have the Combo-Meal • A gas has a volume of 800.0 mL at -23.00 °C and 300.0 torr. What would the volume of the gas be at 227.0 °C and 600.0 torr of pressure?

  11. Avogadro’s Law • Published in 1811 by Amedeo Avogadro, it states that for a gas with a fixed pressure and temperature, the volume of the gas is directly proportional to the number of particles of the gas – we now use moles. • V ∝ n • Generalizing this, we get • V1/n1 = V2/n2

  12. Attack of the Mole • A container with a volume of 18.7 L contains 0.379 mol nitrogen. • How many moles of fluorine must be added to increase the volume to 43.4 L?

  13. Ideal Gas Law (pt 1) • Published in 1834 by Émile Clapeyron based off of Boyle’s Law and Charles’s Law, it states that for an ideal gas, the pressure-volume product is directly proportional to the mole-temperature product. • PV ∝ nT 

  14. Ideal Gas Law (pt 2) • The proportionality constant is the same for all gases! • It is called the Ideal (or Universal) Gas Constant with symbol R. • Adding R, we get • PV = nRT

  15. What’s the Pirate Movie Rated? • R has many possible values. • The 3 most common ones: • If P is in atm, R = 0.08205746 atm·L / mol·K • in kPa, R = 8.314472 kPa·L / mol·K • in mmHg, R = 62.36367 mmHg·L / mol·K (same for torr)

  16. An Ideal Test • What volume will 1.15 moles of H2 occupy at 20.0ºC and 801.8 mmHg?

  17. Universally Yours • At what temperature will 10.967 g of oxygen occupy 0.683 L at 1,266.4 kPa?

  18. Ideal Gases Ideal gases are assumed to consist of: • 1. Randomly moving point particles (no size/volume) that are • 2. Infinitely compressible and • 3. Have no intermolecular attractions (i.e. will not stick to other atoms/molecules)

  19. But Seriously, Folks • Real gases are not point particles. • They have a volume • And they are usually at least two atoms bonded together • (except the noble gases)

  20. Deviation from Ideal • Real gases are not infinitely compressible and • Individual molecules show at least a small amount of attraction to other molecules • This is how we are able to liquefy & solidify gases.

  21. Losing “R” Religion

  22. Approaching the Ideal • Gases exhibit ideal behavior at low pressures and high temperatures (big volumes). • The closest thing to an ideal gas is helium.

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