Semester 2 Exam Review Pd 1

A sample of gas is contained in a closed container under 2 atm of pressure. According to kinetic molecular theory, what causes this pressure?

• The gas molecules are colliding with the walls of the container, exerting a force on the container.

• The gas molecules are colliding with each other, exerting a force on each other.

• The gas particles are chemically reacting with each other releasing energy.

• The gas molecules are attaching to the walls of the container, pulling it inward.

Given the combustion reaction C₃H₈ + 5O₂ ​​→ 3CO₂ + 4H₂O, how many liters of carbon dioxide can be produced from 1.00 liter of O₂ at standard temperature and pressure?

• 0.600 L

• 0.825 L

• 1.21 L

• 1.67 L

Which of the following is not one of the postulates of the Kinetic Molecular Theory for ideal gases?

• The collisions between particles are elastic.

• The particles attract and then repel each other

• The particle size is very small compared to the space between the particles.

• The particles are in constant random motion.

Which graph shows the pressure-temperature relationship expected for an ideal gas?

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Ammonia is produced from the reaction of nitrogen and hydrogen gases. What volume of hydrogen at STP is required to produce 25 g of ammonia?

N₂(g) + 3H₂(g) → 2NH₃(g)

• 33 L

• 1.1 L

• 49 L

• 25 L

Charles' Law States...

• As Pressure goes up volume goes down
• As Pressure goes up temperature goes up
• As Volume goes up temperature goes up 
• As Pressure goes down volume goes down 

Whose law states that as pressure goes up, volume goes down?

• Charles

• Boyle

• Gay-Lussac

• Combined

How do gas molecules move? 

• in an orderly fashion 

• constantly and randomly

• along paths

• in a circular motion

What type of relationship is Charles' Law?

• Inverse
• Direct
• Not enough information
• #goals

True or False: Gases can be compressed. 

• True
• False