Score _____ / 10 pts. Name ____________________________ Class _____ Date ___________________

8.2 Gas Laws Practice – Temperature and Pressure Conversions:

1. The conversion factors for units of temperature are: ◦F = 1.8(◦C) + 32 and K= ◦C + 273

a. Convert 127 ◦F into Kelvin.

b. Convert 127◦ F into ◦ C.

c. Convert 325K into ◦ F.

2. The following equalities relate different units of pressure: 1 kPa = .009869 atm; 1 atm = 101.3 kPa; 760

mmHg = 1 atm; 7.501 mmHg = 1 kPa; 1 torr = 1 mmHg; 1 atm = 14.69596 PSI.

a. Convert 780 mmHg to PSI (pounds per square inch).

b. Convert 350 torr to atm.

c. Convert 15 atm to kPa.

Practice – Gas Laws:

3. (Dalton’s Law of Partial Pressures) Suppose that 5-mL containers of helium (He), neon (Ne), and argon

(Ar) are at pressures of 1 atm, 2 atm, and 3 atm, respectively. The helium and argon gasses are added to

the container of argon.

a. What is the partial pressure of helium in the container after the gases are mixed?

b. What is the total pressure in the container after the three gases are mixed?

Score _____ / 10 pts. Name ____________________________ Class _____ Date ___________________

4. (Boyle’s Law) A diver blows a 0.75 L air bubble 10 m under water. As the bubble rises to the surface, the

pressure of the water decreases from 2.25 atm to 1.03 atm. What will be the volume of the bubble just as

it reaches the surface?

5. (Charles’s Law) A helium balloon in a closed car occupies a volume of 2.32 L at 40.0◦ C. If the car is

parked on a hot day and the temperature inside the car rises to 75.0◦C, what is the new volume of the

balloon, assuming pressure in the car remains constant?

6. (Gay-Lussac’s Law) The pressure of oxygen gas inside a canister is 5.00 atm at 25.0◦C. The canister is

located at a camp high on Mount Everest. If the temperature falls to -10.0◦C, what is the new pressure

inside the canister?

Score _____ / 10 pts. Name ____________________________ Class _____ Date ___________________

7. (Combined Gas Law) A gas at 110 kPa and 30.0◦C fills a flexible container with an initial volume of 2.00 L.

If the temperature is raised to 80.0◦ C and the pressure increases to 440 kPa, what is the new volume?

Practice – Ideal Gas Law:

Pressure Unit Value for Ideal Gas Constant (R)

Atmospheres (atm) .0821 L•atm/(n•K)

KiloPascals (kPa) 8.314 L•kPa/(n•K)

Millimeters of Mercury (mmHg or torr)

62.4 L•mmHg/(n•K)

Equation to MEMORIZE: PV = nRT

P =

V =

n =

R =

T =

8. What volume would be occupied by 100 grams of oxygen gas at a pressure of 1.05 atm and a

temperature of 25 C?

P=

V=

n=

R=

T=

Score _____ / 10 pts. Name ____________________________ Class _____ Date ___________________

9. Calculate the pressure in millimeters of mercury of a 0.323 mole sample of a gas in a 5.6 L container at

155°C.

10. Calculate the volume that 2.00 kg of methane gas will occupy at STP (0°C and 1 atm).

11. An engineer wishes to design a container that will hold 14.0 moles of gas at a pressure no greater than

550 kPa at a temperature of 49°C. What is the minimum volume the container can have?

Score _____ / 10 pts. Name ____________________________ Class _____ Date ___________________

12. (Challenge) Solid iron reacts with water at controlled conditions of 3 atm and 500K to produce .500 L of

hydrogen gas and solid magnetite (Fe3O4). Theoretically, what mass of iron was required to complete the

reaction at the given conditions?

13. Calculate the molar mass of a gas if 2.50 g occupies 0.875 L at 685 torr and 35°C. (Answer: 80.1

g/mol)

14. Calculate the density of NO2 gas at 0.97 atm and 35°C.