Introduction to Kinetic Molecular Theory

A gas that behaves according to all the assumptions of the kinetic-molecular theory

A gas that is found only in laboratory conditions

A gas that cannot be compressed

A gas that exists only at high temperatures

Gas particles are mostly empty space themselves.

Gas particles are in constant motion.

The kinetic energy of gas particles is very high.

Gas particles are extremely small.

Circular motion

constantly and randomly

in an orderly fashion

in straight line paths

Inelastic collisions with energy loss

Elastic collisions with no overall loss of kinetic energy

Partially elastic collisions with some energy transfer

Completely inelastic collisions with total energy loss

Because the particles are too small

Because the particles are in constant motion

Because the particles do not interact thermally

Because the particles are considered independent of each other

It decreases as temperature increases

It remains constant regardless of temperature

It increases as temperature increases

It is independent of temperature

high temperature

low pressure

low temperature

high volume

high pressure

Particles are static and unchanging.

Particles move only when heated.

All particles are always in motion.

Particles do not exist in gases.

They are invisible and can be compressed.

They expand and fill containers.

They are tightly packed and move minimally.

They move freely and quickly.

They are more tightly packed.

They are usually invisible.

They move less and slower.

They have more energy and can move around.

They form a regular pattern.

They can be compressed and expanded.

They are visible to the eye.

They hardly move at all.

Higher temperature reduces particle energy.

Higher temperature increases particle energy.

Lower temperature increases particle energy.

Temperature has no effect on particle energy.