Kinetic Theory of Gases

• Kinetic Energy is energy in motion.

• Higher temperature therefore means more motion​.

• These are shown only by Ideal gases which do not exist.

• Temperature

• Volume

• ​Pressure

Gas Behavior will be impacted by factors to include:​

Factors affecting Gas Behavior

These relationships are expressed in Gas Laws.

When any one of these factors is kept constant, the other two will be affected.. Place finger over any one (representing the constant) and swing stick up or down to see the effect on the others.

The higher the temperature, the greater the Kinetic energy the gas molecules have.

More kinetic energy means more collision, more movement and greater spread in available space.​

At constant volume, as temperature INCREASES the pressure on the gas also INCREASES.

Temperature and pressure are DIRECTLY PROPORTIONAL​.

Temperature

• The larger the space occupied by the gas, the greater its volume.

• Gases usually spread to occupy all the space available. ​

• If the pressure on a gas is constant​, then Increasing temperature, increases volume.

• Therefore, temperature and volume are directly proprotional.​

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Volume

• The smaller the surface area, the greater the pressure.

• If gases are held at a constant temperature, then the pressure on the gas will INCREASE as the Volume DECREASES.

• This is because of the increased force as more particles will start colliding in the walls of the container​.

• TherEfore, Pressure and Volume are INVERSELY PROPORTIONAL.​

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Pressure

CHARLES' LAW

• Involves T and V, constant P.

• Directly Proportional as when one increases the other also increases​.

• ex. car tires in winter appear flatter​

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• Involves P and V with constant T

• Inversely proportional- as one increases the other decreases​.

• ex. ​ear popping in airplane at high altitude. pushing down on a syringe when covered.

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• Involves P and T, constant V.

• Directly Proportional-as one increases the other also increases.

• Ex. ​aerosal can in fire, pressure cooker

​Gay-Lussac law