Directions: Solve the following problems by using the Basic Gas Laws (Boyle, Charles, Gay-Lussac, Combined, and Partial Pressures). Some of these calculations may involve additional conversions using the equations for density, specific heat, etc. Show all of your work, as seen in the example below. Box your answer.

Example: A) Suzy has purchased a 10 kg helium tank to fill balloons for her best friend’s birthday party. Helium’s density is 1.78 x 10-4 g/cm3. What will the final volume of the helium balloons be if she uses all the helium in the tank and the temperature increases during the party from 20C to 33C?

B) How much pressure must the helium tank have originally been under if the total amount at 20C was bottled into a container with a volume of just 9,000 cm3 (assume the new pressure inside the tank is 1 atm)?

1.Decide which gas law to use, based on the information given. Write it down in its original form.

2.Write out all the starting information, in a column.If your units don’t match, convert them until they do.

3.Convert all Celsius temperatures to Kelvin, by adding 273.

4.Rearrange your original equation to solve for the one variable you do not have information for.

5.Plug in your information into the rearranged equation, canceling all units except for the one you need in your answer.

6.Box your answer, with the appropriate unit.

Use the BASIC GASLAWS to solve the following equations:

  1. A gas mix contains oxygen, nitrogen, and carbon dioxide @ 72.9 kPa. If P[O2] = 26.60 kPa, and P[N2] = 13.0 kPa, what is P[CO2] ?
PT = ______
P1 = ______
P2 = ______
P3 = ______?______
  1. A particular gas took up 40.0L of space @ 100C and 0.555atm. If the temp increased by 20C and the pressure changed to 2.33 atm, what would the resulting volume be?
P1 = ______
V1 = ______
T1 = ______C  ______K
P2 = ______
V2 = ______
T2 = ______C  ______K
  1. A sample of gas occupied a volume of 15.0L at a temp of 30.0C. If the temp were to increase by 15C, what would be the volume of the gas under this new condition?
V1 = ______
T1 = ______C  ______K
V2 = ______
T2 = ______C  ______K
  1. A sample of helium in a vacuum system was compressed from a volume of 200.0mL to a volume of 0.240mL where the pressurewas found to be 30.0 mmHg. What was the original pressure of the helium?
P1 = ______
V1 = ______
P2 = ______
V2 = ______
  1. If a sample of a gas has a volume of 5.00L @ 92.3C, what will the volume of the gas be if the temperature is lowered to -37C?
V1 = ______
T1 = ______C  ______K
V2 = ______
T2 = ______C  ______K
  1. The gas left in a used aerosol can is at a pressure of 110 kPa at 18C. If the can is thrown into a fire, what will the pressure be inside the can @ 936C?
P1 = ______
T1 = ______C  ______K
P2 = ______
T2 = ______C  ______K
  1. The volume of a gas-filled balloon is 36.0L @ 49.0C and 152.0 kPa pressure. What volume will the balloon have @ STP?
P1 = ______
V1 = ______
T1 = ______C  ______K
P2 = ______
V2 = ______
T2 = ______C  ______K
  1. When 3.59 L of CO2 at 2.27 atm and 51.0C is heated and compressed, the new pressure is 3.56 atm and the new temp is 104.0C. What is the new volume?
P1 = ______
V1 = ______
T1 = ______C  ______K
P2 = ______
V2 = ______
T2 = ______C  ______K
  1. Using 5.596 L N2 as the initial volume, calculate the volume that would result if the pressure was raised from 100 kPa to 150kPa.
P1 = ______
V1 = ______
P2 = ______
V2 = ______
  1. An 8.1L air sample at a temp of -23C has a pressure of 156 kPa. What will be the new pressure if the temp is raised to 170C and the volume expands to 10.0L?
P1 = ______
V1 = ______
T1 = ______C  ______K
P2 = ______
V2 = ______
T2 = ______C  ______K
  1. A tire has a volume of 2.4 L after is had been heated from 24C to 39 C. What was its original volume?
V1 = ______
T1 = ______C  ______K
V2 = ______
T2 = ______C  ______K