UNIT 8 REVIEW
GAME
Gas Laws
Rules:
•Pick one of the questions to do in each
problem set (1 question per team member).
•Once you finish your question, pass back your
paper to your teammate.
•If you are the last person in your row, check
the work of the people in front of you.
•When you are finished, run your paper back
up to the front!!
Round 1: Gas Concepts
***Pick 1 question/person
Answer the following questions:
1. How does temperature affect particle speed?
2.
Why would adding gas to a container increase
the pressure?
3.
Describe the relationship between (1) P & T,
(2) P & V, and (3) V & T.
4.
What does STP mean? What does it
correspond to?
1) Temperature is a measure of the average kinetic energy. So, the higher
the temperature, the more kinetic energy in the sample. The greater the
kinetic energy, the faster the particles move. 2) Adding a gas to a container will increase the number of molecules
hitting the walls of the container. If there are more collisions, that would
correspond with a higher gas pressure. 3) Pressure & temperature = directly proportional
Volume & temperature = directly proportional Pressure & volume = indirectly proportional (inverse relationship)
4) STP stands for standard temperature and pressure. Standard
temperature is zero degrees Celsius (273 Kelvin); standard pressure is 1
atmosphere (atm).
Round 2: Mixed Gas Laws ***1 question/person
Solve the following problems – show your work!
1.
2.
3.
4.
A 70. liter sample of gas initially at 280°C is allowed to cool at
constant pressure, what will the new volume be at O°C?
It’s not safe to put aerosol canisters in a campfire because the
canisters can explode. If a 1500 mL canister which contains 16.0
grams of hydrogen gas is tossed in a campfire at 1400°C, what is
the pressure inside the canister?
A sample of oxygen gas has a volume of 150 mL when its
pressure is 440 mmHg. If the pressure is increased to 760 mmHg
and the temperature remains constant, what will the new gas
volume be?
At a pressure of 780 mmHg and 24.2°C, a certain gas has a
volume of 350 mL. What will the volume of this gas be at STP?
Round 3: Mixed Gas Laws ***1 question/person
Solve the following problems – show your work!
1.
2.
3.
4.
Seaweed plants release oxygen gas during photosynthesis.
A 0.10 mL bubble is released under water at a pressure of
176 kPa and a temperature of 10°C. What volume will this
bubble occupy at the surface, where the temperature is
15°C and the pressure is 250 kPa?
How many moles of gas are in a scuba tank if the
temperature of the tank is 30°C and the pressure is
200 atm? The volume of the tank is 7 liters.
At a pressure of 405 kPa, the volume of a gas is 6.00 mL.
Assuming the temperature remains constant, at what
pressure will the new volume be 4.00 mL?
What volume will 1 mole of gas occupy at 20°C and
812 mmHg?
Round 4
***1 question/person
1.
If you have 46.0 g of oxygen gas at STP, how much volume
will the oxygen take up?
2.
A 0.24 g sample of a gas occupies a volume of 115 mL at a
pressure of 712 mm Hg and 22°C. What is the molar mass
of this unknown gas?
3.
If you react 3.6 g of KClO3 at STP, how many milliliters of
oxygen gas will you produce? 2 KClO3 ------> 2 KCl + 3 O2(g)
4.
If you want to produce 450 mL of CO2 at a temperature of
23°C and 0.90 atm, how many grams of methane (CH4)
would need to react? Note that the reaction is unbalanced
and not at STP.
___ CH4 (g) + ___ O2 (g)
____ CO2 (g) + ___ H2O (g)
Round 5: Dalton’s Law & Graham’s Law
***Pick 1 question/person
1.
A mixture of oxygen, hydrogen and nitrogen gases exerts
a total pressure of 278 kPa. If the partial pressures of the
oxygen and the hydrogen are 112 kPa and 101 kPa, what
is the partial pressure exerted by the nitrogen?
2.
An unknown gas diffuses 0.25 times as fast as He. What
is the molar mass of the unknown gas?
3.
Which gas will effuse/diffuse slower?
4.
If equal amounts of helium and argon are placed in a
porous container and allowed to escape, which gas will
escape faster and how much faster?
CO or Cl2