Ideal Gas Laws w/s

Please answer all questions on a separate sheet of paper.  Show all work for full credit.

  1. How many moles of gas are contained in 890.0 mL at 21.0 °C and 750.0 mm Hg pressure?
  2. 1.09 g of H2 is contained in a 2.00 L container at 20.0 °C. What is the pressure in this container in mm Hg?
  3. What volume will 20.0 g of Argon occupy at STP?
  4. How many moles of a gas would be present in a gas trapped within a 37.0 liter vessel at 80.00 °C at a pressure of 2.50 atm?
  5. Determine the number of grams of carbon dioxide in a 450.6 mL tank at 1.80 atm and minus 50.5 °C. Determine the number of grams of oxygen that the same container will contain under the same temperature and pressure.
  6. A 40.0 g gas sample occupies 11.2 L at STP. Find the molecular weight of this gas. (hint: # moles = mass/molar mass)
  7. 96.0 g of a gas occupies 48.0 L at 700.0 mm Hg and 20.0 °C. What is its molecular weight?
  8. Calculate the volume 3.00 moles of a gas will occupy at 24.0 °C and 762.4 mm Hg.

Now you need to figure out if the following problems require the ideal gas law or the combined.

  1. At what pressure would 0.150 mole of nitrogen gas at 23.0 °C occupy 8.90 L?
  2. If a gas is initially at 12.5 atm, has a volume of 250 mL, and a temperature of 50.0oC, then the container is raised to a pressure of 14.0 atm and temperature is increased to 75.0oC, what is the new volume in mL?
  3. A gas has a temperature of 14.0oC and a volume of 450. mL. What is the new volume if temperature is raised to 35.0oC and pressure is held constant?
  4. How many grams of Nitrogen gas are contained in a 50.0 L cylinder at a pressure of 100.0 atm and a temperature of 35.0 °C?

Dalton’s Law of Partial Pressures & Graham’s Law

  1. A gas tank contains 152 g of CO2 gas and 86 g of O2 gas at a total pressure of 365 kPa.
  2. How many moles of CO2 are there?
  3. How many moles of O2 are there?
  4. What is the partial pressure of oxygen gas?
  5. What is the partial pressure of carbon dioxide gas?
  6. A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the oxygen is 2.00 atm, and the pressure of carbon dioxide is 3.00 atm. If the total pressure of the container is 8.50 atm, what is the partial pressure of the helium in mmHg?
  7. A container with two gases, helium and argon, is 30.0% by volume helium. Calculate the partial pressures of helium and argon if the total pressure inside the container is 4.00 atm.
  8. Air is a mixture of gases. By percentage, it is roughly 78% nitrogen, 21% oxygen and 1% argon. If the atmospheric pressure is 760 mm Hg, what are the partial pressures of nitrogen, oxygen and argon in the atmosphere?
  9. Blast furnaces give off many unpleasant and unhealthy gases. If the total air pressure is 0.99 atm, the partial pressure of carbon dioxide is 0.15 atm, and the partial pressure of hydrogen sulfide is 0.21 atm, what is the partial pressure of the remaining air?
  10. If the air from problem the last problem contains 22% oxygen, what is the partial pressure of oxygen near a blast furnace?
  11. Which gas effuses faster: oxygen or carbon dioxide? How do you know?
  12. Which gas effuses faster, hydrogen or chlorine? How much faster?
  13. Calculate the ratio of the velocity of helium atoms to fluorine molecules at the same temperature.
  14. Calculate the ratio of the velocity of helium atoms to the velocity of neon atoms at the same temperature.

Extra Credit:

  1. A certain gas effuses 4 times as fast as oxygen. What is the molar mass of the gas?