Name: ______

Period: ______

Date: ______

Gas Laws Test Review Packet

Directions:

1)Solve the following

2)Write the proper equation

3)Show ALL work with units

4)Give the proper answer, with the proper number of significant figures and the proper units

1)Calculate each of the following quantities

  1. The volume of a gas, in liters, if 1.75 moles has a pressure of 748.6 mmHg at a temperature of -6 0C.
  2. The absolute temperature of the gas at which 3.33 x 10-3mol occupies 255 mL at 720 torr.
  3. The pressure, in kPa of 19.6 grams of Nitrogen in a 6.41 liter flask at 0 0C
  4. The pressure in atmospheres if .0467 mol occupies 413 mL at 122 0C
  5. The quantity of gas, in moles, if 67.5 L at 54 0C has a pressure of 11.25 kPa.

2)An unknown vapor has a mass of .846 grams, a volume of 3540 mL, a pressure of 100.23 kPa and a temperature of 100 0C.

  1. The pressure of the vapor is increased to 104.57 kPa, the volume is decreased to 2789 mL and the mass remains constant. What is the new temperature?

3)Calcium hydride, CaH2, reacts with water to form hydrogen gas and calcium hydroxide

CaH2 + H2O Ca(OH)2 + H2

  1. If 20 grams of CaH2 reacts with 35 grams of water, what volume of H2 would be produced in a cylinder that has a pressure of 786 mmHg at a temperature of 18 0C

4)The safety air bags in automobiles are inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3:

NaN3 Na + N2

a)If an air bag has a volume of 36,000 mL and is to be filled with nitrogen gas at a pressure of 874 torr at a temperature of 34 0C, how many grams of NaN3 must be decomposed?

5)Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 65 liters and which contains oxygen gas at a pressure of 16,500 kPa at 23 0C

  1. What volume would the gas occupy at STP
  2. At what temperature would the pressure in the tank equal 150 atm
  3. What would be the pressure of the gas, in kPa, if it were transferred to a container at 44 0C whose volume is 55.0 liters

6)A fixed quantity of gas at 45 0C exhibits a pressure of 735 mmHg and occupies a volume of 5220 mL.

  1. Calculate the volume the gas will occupy if the pressure is increased to 1.88 atm, while the temperature is held constant
  2. Calculate the pressure the gas will occupy if the temperature is increased to 75 0C while the volume is held constant.
  3. Calculate the volume the gas will occupy if the temperature is increased to 165 0C while the pressure is held constant.

7)Solid iron(II) chloride is decomposed to produce solid iron and chlorine gas.

FeCl2 Fe + Cl2

  1. What volume of chlorine has measured at 71.7 0C and 1.33 atm will be produced when 8.4 moles of iron(II) chloride is decomposed?

8)A certain sample of gas occupies a volume of 20.0 L at a temperature of 21˚C and a pressure of 0.89 atm.

  1. How many moles are there in the sample?
  2. If the temperature is increased to 85˚C and the volume is changed to 35.0 L, what is the pressure?

9)A helium-filled weather balloon has a volume of 240 L at 99 kPa pressure and a temperature of 0˚C. What is the mass of the helium in the balloon?

10)What is the volume occupied by 1.24 mol of a gas at 35˚C if the pressure is 96.2 kPa?

11)A sample of nitrogen gas has a pressure of 6.58 kPa at 539 K. If the volume does not change, what will the pressure be at 211 K?

12)The pressure in a car tire is 198 kPa at 27˚C with a volume of 5 L. After a long drive, the pressure is 225 kPa and the volume remains constant. What is the temperature of the air in the tire?

13)A 5.00 L air sample has a pressure of 107 kPa at a temperature of -50.0˚C. If the temperature is raised to 102˚C and the volume expands to 7.00 L, what will the new pressure be?

14)An ideal gas originally at .85 atm and 66 0C was allowed to expand until its final volume, pressure, and temperature were 94 mL, .60 atm, and 45 0C. What was its initial volume?

15)

1. What is Boyle’s Law? What is the relationship between the variables? What condition is held constant?

2. What is Charles’ Law? What is the relationship between the variables? What condition is held constant?

3. What is Gay-Lussac’s Law? What is the relationship between the variables? What condition is held constant?

4. What is the combined gas law? Why would we use this law? *Hint – what condition is held constant?*

5. State the Ideal Gas Law.

6. There are three different R values that can be used in the ideal gas law. How do you know which one to use?

  1. Why does gas pressure decrease when gas is removed from a container with a fixed volume?
  2. If a gas is compressed from 4 L to 1 L and the temperature remains constant, what happens to the pressure?
  3. Describe what happens to the volume of a balloon when it is taken outside on a cold winter day. Explain why the observed change happens.
  4. Explain why heating a contained gas that is held at a constant volume increases its pressure.
  5. What does the abbreviation STP mean? What are the conditions of STP?

Directions:

a)Solve the following problems

b)Write the proper equation

c)Show ALL work with units

d)Give the proper answer with units

1)The base of a box is 12 inches by 10 inches. It weighs 360 pounds. What is the pressure exerted by the box on the floor?

2)What is the weight (force) of an object that has a base which is 4 square inches and exerts a pressure of 25 pounds per square inch?

3)A round tube weighs 30 lbs. If the tube is stood up on one end it pushes down on the floor with a pressure of 3.5 lbs/in2. How many square inches is the tube?