Kinetic Molecular Theory
According to kinetic molecular theory, gas particles are in constant __________ motion.
random.
What causes gas pressure?
Particles hitting the walls of a container.
Boyle’s Law describes the relationship between pressure and what?
Volume
Charles’s Law describes the relationship between temperature and what?
Volume.
What happens to gas particles when temperature increases?
They move faster.
Do gas particles move faster at higher or lower temperatures?
Higher temperatures
If more gas particles are added to a container, what happens to pressure?
Pressure increases
If volume decreases, pressure __________.
increases
If temperature increases, volume __________.
Increases
What law explains squeezing a balloon?
Boyle’s Law
Why do gases spread out to fill their container?
Because particles move freely and constantly in all directions.
If particles move faster, what happens to pressure?
Pressure increases.
What type of relationship is Boyle’s Law?
Inverse relationship
What type of relationship is Charles’s Law?
Direct relationship.
What law explains a balloon expanding in a warm room?
Charles's Law
What happens to particle speed when temperature decreases?
Particles slow down
In a sealed container, what happens to pressure if temperature increases?
Pressure increases.
What must stay constant in Boyle’s Law?
Temperature
What must stay constant in Charles’s Law?
Pressure
If pressure doubles, what happens to volume (temperature constant)?
Volume decreases (is cut in half).
How does kinetic molecular theory explain pressure?
Pressure is caused by gas particles colliding with the walls of the container.
Why does a tire’s pressure increase on a hot day?
The air inside heats up, particles move faster, increasing pressure.
Why is a syringe harder to push when compressed?
Decreasing volume increases pressure.
Why does a balloon shrink in the freezer?
Lower temperature causes volume to decrease.
Explain why aerosol cans warn not to expose to heat.
Heat increases particle speed and pressure, which could cause explosion.