# Gas Laws And Principles: Trivia Quiz!

20 Questions | Total Attempts: 591  Settings  There are different types of gasses in existence, and over the week, we have been able to learn so much more about them and their characteristics. Did you know that compound gasses contain a combination of different atoms? Do you think you have what it takes to answer the question below based on all we learned? Give it a shot and get to find out!

• 1.
TRUE or FALSE. According to Charles Law, if you have a balloon inside a car at noon during a hot summer day the balloon molecules inside will increase in pressure.
• A.

True

• B.

False

• 2.
In a nitrogen gas occupies has a volume of 500ml at a pressure of 0.971atm.What volumewill the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?
• A.

342mL

• B.

424mL

• C.

324mL

• D.

442mL

• E.

242mL

• 3.
Not all Gas Law problems have Kelvin (K) as the unit of temperature. They can be expressed in Celsius (°C)and Fahrenheit(°F). So convert 123°C to K.
• A.

396K

• B.

486K

• C.

369K

• D.

458K

• E.

693K

• 4.
Gas pressure is caused by
• A.

Gas molecules heating up

• B.

Gas molecules reacting with other gas molecules

• C.

Gas molecules hitting the walls of a container

• D.

Gas molecules hitting other gas molecules

• 5.
At a pressure of 5.0 atmospheres, a sample of gas occupies 40. liters. What volume will the same sample occupy at 1.0 atmosphere?
• A.

0.0050 L

• B.

0.13 L

• C.

200 L

• D.

8.0 L

• 6.
As the volume of confined gad decreases at constant temperature, the pressure exerted by the gas ______.
• A.

Decreases

• B.

Increases

• C.

Stay the same

• D.

Fluctuates

• 7.
A sample of argon has a volume of 0.43 mL at 299K. At what temperature in degrees Celsius will it have a volume of 1 mL.
• A.

695°C

• B.

422°C

• C.

428°C

• D.

694°C

• 8.
Each of these flasks contains the same number of molecules. In which container is the pressure highest?
• A.

• B.

• C.

• D.

• E.

• 9.
TRUE or FALSE: A good example of Charles Law is when a piece of metal expands in the heat
• A.

True

• B.

False

• 10.
Assuming that the temperature remains constant. How can you increase the pressure of a gas?
• A.

Increase the container volume

• B.

Add more molecules of the gas

• C.

Decreases the container volume

• D.

None of the above

• 11.
In a closed container at 1.0 atmosphere, the temperature of a sample of gas is raised from 300 K to 400 K. What will be the final pressure of the gas?
• A.

0.010 atm

• B.

0 atm

• C.

100 atm

• D.

1.3 atm

• 12.
At constant pressure and 25 °C a sample of gas occupies 4.5 liters. At what temperature will the gas occupy 9.0 liters?
• A.

596K

• B.

50K

• C.

50°C

• D.

596°C

• 13.
TRUE OR FALSE. You drove continuously from Laguna to Manila and you observed that the pressure in your tires increased. This is because of the increased temperature outside the tire caused by friction.
• A.

True

• B.

False

• 14.
Each of these flasks contains the same number of gas molecules. In which would the pressure be lowest?
• A.

• B.

• C.

• D.

• 15.
Neon gas has a volume of 2,000ml with an atm of 1.8 however the pressure decreased to 1.3atm what is now the volume of the neon gas?
• A.

2, 795mL

• B.

2,759mL

• C.

3,795mL

• D.

3,759mL

• 16.
Each of these flasks is the same size and at the same temperature. Which one contains the most molecules?
• A.

• B.

• C.

• D.

• 17.
When a supply of hydrogen gas is held in a 4 liter container at 320 K it exerts a pressure of 800 torr. The supply is moved to a 2 liter container, and cooled to 160 K. What is the new pressure of the confined gas?
• A.

800 torr

• B.

1600 torr

• C.

200 torr

• D.

400 torr

• 18.
Which Gas Law is involved when a balloon pops after being sat on?
• A.

Charles Law

• B.

Boyle's Law

• C.

• D.

None of the Above

• 19.
A small sample of helium gas occupies 6 mL at a temperature of 250 K. At what temperature does the volume expand to 9 mL?
• A.

125K

• B.

375K

• C.

500K

• D.

2250K

• 20.
Organize the following gases in order of their rates of difusion, from slowest to fastest oxygen, O2 ammonia, NH3 hydrogen, H2 carbon dioxide, CO2
• A.

Hydrogen, oxygen, carbon dioxide, ammonia

• B.

Oxygen, hydrogen, carbon dioxide, ammonia

• C.

Hydrogen, ammonia, oxygen, carbon dioxide

• D.

Hydrogen, oxygen, ammonia, carbon dioxide

• E.

Carbon dioxide, oxygen, ammonia, hydrogen

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