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# F4.4.4 gas law

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### F4.4.4 gas law

1. 1. UNDERSTANDING THE GAS LAWS <br />
2. 2. GAS LAWS <br />
3. 3. GAS LAWS <br />
4. 4. Boyles’s Law<br />For a fixed mass of gas, the pressure of the gas, P is inversely proportional to its volume, V when the temperature, T is kept constant<br />
5. 5. Boyle’s Law <br />
6. 6. When the volume<br /> of a gas is decreased<br /> the number of<br /> molecules per unit volume increases. <br />The same number of molecules moves in a smaller space. <br />•The molecules collide more frequently with the walls of the container. <br />This increase in the rate of collision results in an increase in the pressure exerted by the gas. <br />
7. 7. Charles’ law<br />For a fixed mass of gas, the volume of the gas, V is directly proportional to its absolute temperature, T when its pressure, P is kept constant<br />
8. 8. Charles’ law<br />
9. 9. When a gas is heated, the average kinetic energy of the molecules increases. The temperature of the gas increases. <br />The rate of collision between the molecules and the walls will increase if the volume is constant. <br />It the gas is allowed to expand, the faster molecules now move in a bigger space. <br />Therefore, the rate of collision between the molecules and the walls remain constant and thus the pressure is constant <br />
10. 10. Pressure’s Law<br />For a fixed mass of gas, the pressure of the gas, P is directly proportional to its absolute temperature, T when its volume, V is kept constant.<br />
11. 11. Pressure’s Law<br />
12. 12. When a gas is heated, the average kinetic energy increases. The temperature of the gas increases. <br />• The faster moving molecules strike the walls of the container more frequently. <br />• Thus, the pressure of the gas increases. <br />Pressure’s Law<br />
13. 13. Experiments <br />
14. 14. Manipulated: Volume of air in a syringe <br />Responding: Pressure of trapped air <br />Fixed : mass and temperature of air inside a syringe <br />
15. 15. Manipulated:<br /> Temperature of trap air <br />Responding: <br />Length of air column<br />Fixed : atmospheric<br /> pressure, Mass of trapped air <br />The length of the air column, x represents the volume of air trapped inside the capillary tube. <br />The pressure of the trapped air = <br />atmospheric pressure + pressure<br />due to the concentrated acid <br />
16. 16. Manipulated: Temperature of trap air <br />Responding: Pressure of the trapped air <br />Fixed : Volume of air <br />Mass of trapped air <br />
17. 17. Absolute temperature <br />Tem peraturesmeasured in the Kelvin, K scale. <br />Convert °C to Kelvin: θ + 273 <br />Convert Kelvin to °C : T – 273 <br />
18. 18. Absolute zero <br />The lowest possible temperature which is -273°C or 0 K<br />0K = -273 °C<br />At this point:<br />Voumeand pressure of gas is zero <br />Kinetic energy of the gas molecules is zero <br />Gas molecules are stationary. <br />
19. 19. THE END<br />