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Warm-up

Warm-up. I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60 atm. If by increasing the temperature to 225 K and decreasing the pressure to 30 atm causes the volume of the gas to be 29 liters, how many liters of gas did I start with?.

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Warm-up

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  1. Warm-up • I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60 atm. If by increasing the temperature to 225 K and decreasing the pressure to 30 atm causes the volume of the gas to be 29 liters, how many liters of gas did I start with?

  2. The Ideal Gas Law Unit 8, Day 7 Kimrey 4 December 2012

  3. A Bit More About Gases • Remember gases are really tiny particles bouncing off of everything. • These collisions are perfectly elastic. Meaning that no energy is lost as they collide. • It’s because of this that the combined gas law works (P1V1/T1 = P2V2/T2).

  4. Adding more gas • So what happens if we add more of a gas? • This can be accounted for by the ideal gas law.

  5. Ideal Gas Law PV=nRT • P= Pressure • V= Volume • n= moles • R= gas constant • T= Temperature

  6. Units • Temperature must be in Kelvin. • Volume must be in liters (Remember: King Henry Died by drinking chocolate milk) • Pressure can be in atm, mmHg, or kPa BUT you must use the appropriate R for whatever units of pressure you have. • R is a constant and can be: (three options are found on the reference tables)

  7. Converting to Kelvin • Temperature can also be measured in a unit known as Kelvin. • Degrees Celsius plus 273 = Temperature in Kelvin • You don’t have to remember this! The reference tables show that 0 °C is the same as 273K • 45°C is what in Kelvin? • 5°C is what in Kelvin?

  8. Example • How many moles of a gas at 100°C does it take to fill a 1.00L flask to a pressure of 1.50 atm?

  9. Example • If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?

  10. Example • If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, how many atmospheres of pressure are inside the container?

  11. Example • If I have an unknown quantity of N2held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many grams of N2do I have?

  12. Warm-up • If I have an unknown quantity of N2 held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many grams of N2 do I have?

  13. Stoichiometry!! Unit 8, Day 7 Kimrey 4 December 2012

  14. Molar Volume • 1 mole = 22.4 L of a gas at STP • STP = 0°C and 1 atm

  15. Examples • How many liters of Nitrogen gas are there in 4.56 moles? • How many liters of fluorine are there in 56.7 grams?

  16. Stoichiometry…Again! N2 + H2 NH3 • 64.0 L of nitrogen will produce how many liters of ammonia (at STP)? • Don’t forget to balance!!!

  17. Mole - Volume 2H2 + O2 2H2O • How many liters of water will be produced from 15 moles of oxygen?

  18. Mass - Volume 2H2 + O2 2H2O • How many liters of water will be produced from 100 grams of Hydrogen gas if Oxygen gas is in excess?

  19. STP • Standard Temperature and Pressure • 1 atm and 0 °C

  20. Example • In a laboratory experiment, 85.3 moles of a gas are collected at 24 °C and 733 mm Hg pressure. Find the volume at STP.

  21. Not at STP… • Use the ideal gas law to determine volume • Then use that volume to complete the stoichiometry

  22. Example Na3PO4 + 3 KOH  3 NaOH + K3PO4 • If you have 25 moles of KOH at 175 K and 3.4 atm, how many liters of K3PO4 are produced?

  23. Example C3H6O + 4 O2 3 CO2 + 3 H2O • At 823 mmHg and 329 K, 135 moles of oxygen are mixed with excess C3H6O. How many liters of water are produced?

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