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# Kinetic Theory Of Gas

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### Transcript

• 1. Gas Law
Kinetic Theory of Gases
• 2. Gas in closed container
Number of molecules is constant
Mass of gas is constant
Behavior of the gas depends on properties of gas
• 3. Properties of Gas
Volume
Molecules move freely and fill the whole space
Gas volume = container volume
Temperature
Average kinetic energy of molecules is proportional to the temperature
• 4. Properties of Gas (cont)
Pressure
When the molecules collide and bounce back, there is a change in momentum
Force is exerted on the wall
Force per unit area is the pressure of the gas
• 5. Relationship Between Pressure and Volume
When the volume decrease, the number of molecules per unit volume increases.
Same number of molecules will move in a smaller space
Molecules collide more frequently with the walls of container.
Thus, pressure will increase
• 6. Boyle’s Law
For a fixed mass of gas, the pressure of the gas is inversely proportional to its volume when the temperature is kept constant.
P α 1/V
PV = constant
P1V1 = P2V2
• 7. Example
The air in a syringe has an initial volume of 12.0 cm3 and pressure of 100 kPa. The nozzle of the syringe is closed and the piston is pushed inwards until the volume of the air becomes 7.5 cm3. What is the pressure of the compressed air in the syringe?
• 8. Solution
P1 = 100 kPa
V1 = 12.0 cm3
P2 = final pressure
V2 = 7.5 cm3
Using Boyle’s law,
P1V1 = P2V2
P2 = P1V1/ V2
P2 = (100 × 12.0) / 7.5
P2 = 160 kPa