KMT and Gas Laws

Which one of these is NOT an Ideal Gas Assumption?

• Gas particles are hard, round spheres.

• Gas particles are strongly attracted to one another.

• Gas particles do not take up space.

• Gas particles collide perfectly elastically.

Which of the following is an assumption of the kinetic-molecular theory of gases?

• Collisions between gas particles are inelastic.

• Gases consist of closely spaced particles.

• Gas particles move around in an orderly manner.

• The temperature of a gas depends on the average kinetic energy of the gas particles.

Which picture best illustrates the particle arrangement in a gas?

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The movement of gas molecules is greatly affected by _________.

• the shape of the container
• size of the container
• temperature of the container

Tags

NGSS.HS-PS3-2

NGSS.HS-PS3-4

Gas molecules can easily be compressed  because ___________. 

• gas molecules are soft

• gas molecules are far apart from each other

• gas molecules takes the shape of the container

• gas molecules collide to lose their kinetic energy

If you place a balloon in a freezer what happens to the size of the balloon?

• Doubles
• increases
• decreases
• stays still

Tags

NGSS.MS-PS1-4

Which is NOT an assumption made by the kinetic molecular theory of gases?

• Gas particles are small and take up little volume
• Particles travel in constant, random, straight-line motion until colliding
• When particles collide, their total kinetic energy is decreased
• Particles do not attract or repel each other

Gas pressure is caused by

• gas molecules colliding with surfaces
• gas molecules condensing to a liquid
• gas molecules hitting other gas molecule
• barometers

Tags

NGSS.HS-PS3-2

Temperature is a direct measure of:

• The density of the particles within a substance.

• The average speed of the particles within a substance.

• How often the particles collide with the walls of their container.

This graph is an example of two variables that are:

• directly proportional
• inversely proportional
• Straight line
• No relation