Chemistry (Practice Test) Name
Chapter 12 (The Gas Laws)
Short Answer
1. Identify the four factors that affect gases. (4pts.)
a.
b.
c.
d.
Matching: Match the name of the gas law with the equation.
A. Boyles Law
B. Charles’s Law
C. Gay-Lussac’s Law
D. Combined Gas Law
E. Ideal Gas Law
F. Dalton’s Law of Partial Pressure
G. Graham’s Law
2. PT = P1 + P2 + P3 + ... Pn
3.
4. P1V1 = P2V2
5. PV = nRT
6. or
7.
8.
9. Identify STP: standard temperature ______standard pressure ______
(Don’t forget the label)
10. At what point during the process of cooling do the Gas Laws become ineffective? (1 pt)
Essay
11. Use the Kinetic Theory to describe why a decrease in the volume of a gas will cause an increase in pressure as stated by Boyles Law.
Multiple Choice (Choose the best answer. 1 pt. each)
_____ 12. Which of the following laws shows and inverse relationship between
pressure and volume?
a) Boyle’s Law b) Charles’s Law c) Graham’s Law d) Dalton’s Law
_____ 13. Which of these laws compares the rates of two gases?
a) Boyle’s Law b) Charles’s Law c) Graham’s Law d) Dalton’s Law
_____ 14. Identify the Gas Law used if the pressure was held constant.
a) Boyle’s Law b) Charles’s Law c) Graham’s Law d) Dalton’s Law
_____ 15. What would happen to the pressure exerted by a gas if the volume is
decreased and the temperature was held constant?
a) The pressure would increase.
b) The pressure would decrease.
c) The pressure would remain unchanged.
_____ 16. In order to solve problems using Charles’s Law or the Combined Gas Law the temperature must be measured in:
a) Fahrenheit b) Celsius c) Kelvin d) Kitzmann
_____ 17. Which of these changes would NOT cause an increase in the pressure of a gaseous system?
a. The container is made larger.
b. Additional amounts of the same gas are added to the container.
c. The temperature is increased.
d. Another gas is added to the container.
_____ 18. What happens to the temperature of a gas when it is expanded quickly?
a. The temperature increases. b. The temperature does not change.
c. The temperature decreases.
_____ 19. What happens to the pressure of a gas inside a container if the temperature of the gas is lowered?
a. The pressure increases. b. The pressure does not change.
c. The pressure decreases.
_____ 20. As the temperature of the gas in a balloon decreases _____.
a. the volume increase. b. the average kinetic energy of the gas decreases
c. the pressure increases d. All of the above
_____ 21. If a balloon is squeezed, what happens to the air pressure within the balloon?
a. It increases. b. It stays the same. c. It decreases.
_____ 22. Which of the following molecules would have the greatest velocity if each gas had the same kinetic energy? Hint: Consult periodic table
a. bromine (Br2) b. chlorine (Cl2) c. ammonia (NH3) d. hydrogen (H2) e. argon (Ar)
Chemistry (Practice Test) Name
Chapter 12 (The Gas Laws)
Word Problems: Solve Show knowns and unknown, Equation used, Substitution, Answer with units.
Draw a box around your answer
1. A gas sample has a volume of 300.0 L when under a pressure of 55.0 kPa. What is the new volume if the pressure is increased to 165 kPa while the temperature is held constant?
2. A quantity of gas occupies a volume of 804 mL at a temperature of 27 °C. At what temperature will the volume of the gas be 402 mL, assuming that there is no change in the pressure?
3. The gas in a closed container has a pressure of 3.00 x 102 kPa at 30°C. What will the pressure be if the temperature is lowered to –172.0°C?
4. A 100 L sample of gas is at a pressure of 80 kPa and a temperature of 200 K. What volume does the same sample of gas occupy at STP?
5. What is the pressure of a 5.0 L container which contains 3.0 moles of a gas at a temperature of 0°C? Note: Use Ideal gas law. R=8.31 (kPa x L)/(mol x K)
6. What volume does 14.0 g of Hydrogen gas (H2) take up at a temperature of 30°C and a pressure of 120 kPa? Note: Use Ideal gas law. R=8.31 (kPa x L)/(mol x K)
7. Two gases CH4 and SO2 are released at the same time from opposite ends of the room. You are in the center of the room. Which gas will reach you first? (hint: mass of S=32; C=12; O=16; and H=1.0)
Part A:
Circle one: Methane (CH4) or Sulfur dioxide (SO2)
Part B: How much quicker will the gas reach you? (Show Your Work for prob. 7 below)
8. A balloon contains 3 different gases (hydrogen, oxygen, and carbon dioxide). If the balloon occupies a volume of 1.0 L , hydrogen gas has a pressure of 100 kPa, oxygen has a pressure of 85 kPa and carbon dioxide has a pressure of 115 kPa. What is the total pressure of the gases exerted on the balloon? (5 pts.)
9. Given a 32.0 g sample of methane gas (CH4) , determine the pressure that would be exerted on a container with a volume of 850 cm3 at a temperature of 30 °C. Note: Carbon = 12.0 and Hydrogen = 1.0
10. Given the following balanced equation.
N2(g) + 3H2(g) ® 2NH3(g)
What volume of ammonia gas (NH3) would be produced at 95.0 kPa and 70 °C if you were given a 28.0 g sample of nitrogen gas (N2)? Note: Nitrogen = 14.0 and Hydrogen = 1.0