KMT, Phase Changes, & Gas Laws

According to the kinetic molecular theory, a gas consists of molecules in constant fixed motion.

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According to kinetic molecular theory-Gas molecules influence each other only by collision; they exert no other forces on each other.

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• False

According to the kinetic molecular theory, all collisions between gas molecules are inelastic; all kinetic energy is lost.

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• False

According to the kinetic molecular theory, the volume actually occupied by the molecules of a gas is negligibly small; the vast majority of the volume of the gas is empty space through which the gas molecules are moving.

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In the KMT, pressure is the force exerted against the wall of a container by the continual collision of molecules against it.

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• False

The total kinetic energy of a collection of gas molecules is inversely proportional to the absolute temperature of the gas.

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• False

Real gases (in real life), like to have high temperatures and low pressures. They like to be warm and free flowing.

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• False

Ideal gases (best conditions) are light molecules such as hydrogen and helium. Heavier gases do not follow this rule.

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• False

Real gases have attraction to other gas molecules which is opposite of the kinetic molecular theory. This way they can have a chemical reaction with each other.

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• False

Gases like to be in very cold conditions and highly pressurized (just like you).

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• False