The kinetic molecular theory (KMT) is a model or theory that is used to explain the behavior of gasses. This Theory describes the relationships among pressure, temperature, velocity, frequency, and force of collisions.
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The Phase of Gas
Gas is spread out indefinitely unless they are confined in a container. In a closed container, the gaseous particles always expand to fill the volume of the container.
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Gas molecules collide with the walls of their container. These collisions with the container wall exert a force over the surface area of a wall - the particles exert pressure on the wall.
As the number of air particles increases ↑, pressure increases ↑ as well.
Pressure and the number of gas molecules are directly proportional.
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The volume and pressure are indirectly related.
If one of the variables (volume or pressure) increases ↑, the other must decrease ↓.
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Temperature of a substance is defined as a measure of the average kinetic energy of its particles.
The kinetic energy Formula:
As temperature rises the kinetic energy increases, due to an increase in velocity.
As the temperature rises, the velocity of the particles increases, causing them to hit walls of the container more often and with greater force. Thus an increase in temperature causes the pressure to increase.
Pressure and temperature are directly proportional.
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The relationships among pressure temperature and volume can be mathematically presented by an equation known as the combined gas law
This model can be used to solve problems of gas properties including, temperature, volume, and pressure, whenever two more of these properties are involved.
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