12.2 Review
The Gas Laws
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Name________________________________
Period_______Date_____________________
1. The pressure of a gas is inversely proportional to its volume. A. Avogadro
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2. The sum of the partial pressures of gases in a mixture is equal
to the total pressure of the mixture.
3. Equal volumes of gases contain equal numbers of particles.
B. Charles Law
C. Boyle’s Law
_______ 4. The volume of a gas is directly proportional to its temperature. D. Dalton’s Law
Match each of the relationships given below with the appropriate graph. Each letter can be used once, more than once, or not at all.
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A B
5. the relationship between gas pressure and its temperature
6. the relationship between gas volume and its pressure
7. the relationship between gas temperature and volume
8. the relationship between gas volume and its molar mass
C
Complete the following statements by writing “decreases,” “increases,” or “remains the same” on the line provided.
As a gas is compressed in a cylinder…
9. the distance between the gas molecules _________________________________________________.
10. the number of gas molecules _________________________________________________________.
11. its volume ________________________________________________________________________.
12. its pressure _______________________________________________________________________.
13. its density ________________________________________________________________________.
14. its mass__________________________________________________________________________.

Complete the following sentences by filling in the correct numerical value.
15. Standard temperature is ______________ degrees Celsius.
16. Absolute zero is ___________________ Kelvin.
17. The volume of 1 mole of any gas at STP is _____________________L.
18. Standard pressure is equal to ________________________kPa.
19. If the pressure of 2 L of a gas at STP doubles, its new volume would be ____________________ L.
20. If the Kelvin temperature of 2 L of a gas at STP doubles, the new volume would be ___________ L.
21. How did Jacques Charles know about the behavior of gases at very low temperatures when he could
not experiment with temperatures below freezing.
22. Use gas law calculations as evidence to describe what happens to an “empty” 200. mL aerosol can at
room temperature (22°C) when it is thrown into an 800. °C fire.
23. If 4.0 L of helium are released into a weather balloon at sea level (pressure = 101 kPa), to what
volume does the balloon expand as it rises to an altitude of 20. km (pressure = 8 kPa)?