Gas Laws: Boyles, Charles, etc / Name:
Period: / ______
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  1. A sample of carbon dioxide occupies a volume of 3.50 liters at 125 kPa. What pressure would the gas exert if the volume was decreased to 2.00 liters?
  1. Ammonia gas occupies a volume of 450. mL at a pressure of 720. mmHg. What volume will it occupy at standard pressure?
  1. Chlorine gas occupies a volume of 1.2 liters at 720 torr pressure. What volume will it occupy at 1 atm pressure?
  1. Fluorine gas exerts a pressure of 900 torr. When the pressure is changed to 1.50 atm its volume is 250. mL. What was the original volume?
  1. A sample of nitrogen gas occupies a volume of 250. mL at 25°C. What volume will it occupy at 95°C?
  1. Oxygen gas is at a temperature of 40°C when it occupies a 2.3 L. To what temperature should it be raised to occupy a volume of 6.5 L?
  1. A sample of argon gas is cooled and its volume went from 380 mL to 250 mL. If its final temperature was -55°C, what was its original temperature?
  1. Hydrogen gas was cooled from 150°C to 50°C. Its new volume is 75 mL. What was the original volume?
  1. A 1.70 mole sample of 02 under 2.00 atm occupies 500 ml at 25 °C.
  1. What will the pressure of the sample be at 0 °C?
  1. What temperature will be needed to produce a pressure of 4.00 atm?
  1. What volume will the gas occupy with 2.6 moles?
  1. How many moles are in a sample that occupies 1.45 L?
  1. How many moles would be needed to have a pressure of 720 mm Hg?
  1. What would be the new pressure if the number of moles was increased to 5.10?

Combined Gas Law

The five gas laws that you have learned thus far can be combined into a single mathematical expression known as the Combined Gas Law. For a given gas law problem involving the changed in one of the 4 variables, simply cancel out any constant and solve.

Write the Combined Gas Law Below:
  1. A certain gas at 25°C and 1.00 atm pressure fills a container of 5.0 L. What volume will the gas occupy at 50°C and 1.05 atm pressure?
  1. Suppose a gas is kept in a sealed container, but the pressure of the gas is increased from 1.00 atm to 1.13 atm. This is done by changing the temperature of the gas from 0°C to a higher temperature. What is this new temperature in °C?
  1. A certain gas occupies a volume of 3.0 L at 25°C and 4.0 atm. What will the volume be at 25°C and 2.0 atm?
  1. A balloon is filled with a gas to a volume of 400. mL at a pressure of 760. mmHg at 25.0°C. The temperature is increased to 50.0°C and the pressure to 1.03 atm. What is the new volume?
  1. Assume that your lungs can hold about 500 mL of air at 0°C and 1.00 atm. You take a deep breath and hold it, then dive into the ocean to a depth at which the temperature is 10°C and the pressure is 1003 mmHg. What is the volume of the air in your lungs?
  1. A gas has a volume of 400. mL at a pressure of 304 kPa and a temperature of 127°C. What would the volume be at 760. mmHg and 273 K?
  1. The volume of a sample of gas is 200. mL at 275 K and 92.1 kPa. What will the new volume be of the gas at 350 K and 0.972 atm?
  1. When 3.5 L of carbon dioxide gas at 2.90 atm and 56°C is heated and compressed, the new pressure is 3.0 atm and the new temperature is 109°C. Find the new volume.
  1. If a sample of gas has a volume of 0.100 L when the pressure is 150. kPa, what is the volume when the pressure is increased to 1.97 atm?
  1. A gas occupies a volume of 473 mL at 36°C. What will be the volume of the gas when the temperature is raised to 94°C?

Ideal Gas Law

The ideal gas law relates the variables that describe a gaseous system at a constant state (no changes).

Write the Ideal Gas Law Below: / R = Universal Gas Constant
0.0821
  1. At what temperature will 7.0 moles of helium gas exert a pressure of 1.2 atm in a 25.0 L tank?
  1. A 500 gram block of dry ice vaporizes to a gas at room temperature. Calculate the volume of gas produced at 25°C and 975 kPa.
  1. If 40 grams of methane, CH4, is confined to 2500 mL at 200°C, what pressure does it exert?
  1. Calculate the volume of 1 mole of CO2 at STP.
  1. How many moles of NH3 are needed to exert a pressure of 3.00 atm in a 5.00 L container with a temperature of 45°C?
  1. How many moles of oxygen will occupy a volume of 2.5 L at 1.2 atm and 25°C?
  1. At what temperature will 5.00 grams of Cl2 exert a pressure of 900. torr at a volume of 750 mL?
  1. What pressure will be exerted by 25 grams of carbon dioxide at a temperature of 25°C and a volume of 500 mL?
  1. Find the number of grams of carbon dioxide that exert a pressure of 785 torr at a volume of 32.5 L and a temperature of 32°C.
  1. A sample of an elemental gas has a mass of 10.3 grams. If the volume of the sample is 58.4 L at a pressure of 758 torr and a temperature of 2.5°C, what is the identity of the gas?

Dalton’s Law of Partial Pressures

Dalton’s Law says that the sum of the individual pressures of all of the gases that make up a mixture is equal to the total pressure. The partial pressure of each gas is equal to the mole fraction of each gas multiplied by the total pressure.

PT = P1 + P2 + P3 … / x PT = Py
  1. A 250. mL sample of oxygen is collected over water at 25°C and 760.0 torr. What is the pressure of the dry gas alone? (vapor pressure of water at 25°C = 23.8 torr)
  1. A 32.0 mL sample of hydrogen is collected over water at 20.0°C and 750.0 torr. What is the volume of the dry gas at STP? (vapor pressure of water at 20°C = 17.5 torr)
  1. A 54.0 mL sample of oxygen is collected over water at 23°C and 770.0 torr. What is the volume of the dry gas at STP? (vapor pressure of water at 23°C = 21.1 torr)
  1. A mixture of 2.00 moles of H2, 3.00 moles of NH3, 4.00 moles CO2, and 5.00 moles of N2 exerts a total pressure of 800. torr. What is the partial pressure of each gas?
  1. The partial pressure of F2 in a mixture of gases where the total pressure is 1.00 atm is 300 torr. What is the mole fraction of F2?