Easy!
Which of the following is a primary assumption of the Kinetic Molecular Theory regarding the volume of gas particles?
The volume of the gas particles themselves is negligible compared to the total volume of the container.
How does the average kinetic energy of gas particles change as the temperature of a gas increases?
It increases.
Why does KMT fail to accurately predict the behavior of gases at very high pressures and very low temperatures?
Because KMT assumes no intermolecular forces and negligible particle volume, which become significant under these conditions.
True or False: According to the Kinetic Molecular Theory, the average kinetic energy of gas particles is directly proportional to the temperature of the gas in Kelvin.
True
If you leave a bottle of perfume open in a room, the scent eventually reaches people on the other side. Which property of gas particles, as described by KMT, explains this?
Diffusion (or random motion).
In the Kinetic Molecular Theory, collisions between gas particles are described as "elastic." What does this mean?
There is no net loss of total kinetic energy during a collision.
According to KMT, why do gases exert pressure on the walls of their container?
Because of the constant, random motion and collisions of particles with the container walls.
At constant temperature, if the pressure of a gas is doubled, what happens to the volume according to the molecular model?
The volume is halved.
True or False: In an "elastic" collision between two gas particles, the total kinetic energy of the system decreases because some energy is converted into heat.
False. In an elastic collision, there is no net loss of total kinetic energy; the total energy of the system remains constant.
In the Kinetic Molecular Theory, what do we call the state of matter where particles have the most freedom of movement?
Gas
If you have a balloon and you heat it up, it expands. Which relationship described by KMT explains this?
Charles's Law
Using KMT, explain what happens to the frequency of collisions with container walls if the volume of a gas is decreased at constant temperature.
The frequency of collisions increases.
If you have a mixture of different gases in a container at the same temperature, which statement is true?
All gas particles have the same average kinetic energy.
True or False: Gas particles in a container are considered to have a significant volume relative to the space between them.
False. The Kinetic Molecular Theory assumes that the volume of the individual gas particles is negligible compared to the total volume of the container.
True or False: Gas particles travel in curved paths because they are constantly being pulled by gravity.
False.
According to KMT, what happens to the velocity of gas particles if the molar mass of the gas increases (assuming constant temperature)?
The velocity decreases.
Two gases, Gas A and Gas B, are at the same temperature. Gas A has a lower molar mass than Gas B. Which gas will diffuse faster?
Gas A
A scientist observes that a real gas deviates from ideal behavior under extreme conditions. Using KMT, which gas would you expect to behave most like an ideal gas?
Helium (noble gas, extremely weak attractions, very small size)
True or False: At a constant temperature, if the volume of a gas is decreased, the gas particles will collide with the walls of the container more frequently.
True
Why does a balloon shrink when you take it from a warm room into a cold freezer?
The particles move slower and hit the walls with less force and frequency, leading to a smaller volume.
Which state of matter is best described by the Kinetic Molecular Theory assumptions of "particles in constant motion" and "high energy"?
Gas
Why can gases be compressed easily, while solids and liquids cannot?
Because there is a large amount of empty space between gas particles.
Based on the Kinetic Molecular Theory, explain the mechanism behind the cooling effect that occurs during evaporation.
The fastest-moving molecules escape the surface, leaving behind slower-moving molecules, which lowers the average kinetic energy.
True or False: Real gases behave most like "ideal" gases under conditions of high pressure and low temperature.
False. Real gases behave most like ideal gases at high temperatures and low pressures, where intermolecular forces are weak and particle volume is negligible compared to the container size.
If you compare a gas to a solid, in which one are the intermolecular forces (attractions) strongest?
In a solid.