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# 3.2 Notes

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### 3.2 Notes

1. 1. Ch 3-2 The Gas Laws <ul><li>Changes in the </li></ul><ul><li>volume, </li></ul><ul><li>temperature, </li></ul><ul><li>pressure, </li></ul><ul><li>and the number of particles </li></ul><ul><li>have predictable effects on the behavior of gases </li></ul>
2. 2. Pressure <ul><li>Pressure is the result of a force distributed over an area </li></ul><ul><li>Newton’s measure force (N) </li></ul><ul><li>Area is square meters </li></ul><ul><li>N/m 2 is called a Pascal or Pa </li></ul><ul><li>Collisions between particles of gas and the walls of a closed container cause pressure </li></ul>
3. 3. Factors Effecting Gas Pressure <ul><li>Temperature- </li></ul><ul><ul><li>Raising the temperature of a gas in a closed container will increase the pressure </li></ul></ul><ul><li>Reducing the volume of the container a gas will increase pressure </li></ul><ul><li>Increasing the amount of gas in a closed container will increase pressure </li></ul>
4. 4. Charles Law <ul><li>Jacque Charles 1746-1823 </li></ul><ul><li>The volume of a gas is directly proportional to its temperature if the pressure and number of particle remain constant </li></ul><ul><li>Absolute zero is 0 Kelvin (K)- 0 o C = -273.15 K </li></ul>As temperature goes up the volume goes up
5. 5. Charles law V V Temperature must be expressed in degrees Kelvin or the volume will not be directly proportional As temperature goes up the volume goes up T T = 1 1 2 2
6. 6. Boyles Law <ul><li>Robert Boyle 1627 </li></ul><ul><li>The volume of a gas is inversely proportional to its pressure if the temperature and number of particles are constant </li></ul><ul><li>P 1 V 1 =P 2 V 2 </li></ul>As Pressure goes up  Volume goes down & Vise-versa
7. 7. Combined Gas Laws <ul><li>PV = PV </li></ul>T T 1 1 1 2 2 2 <ul><li>Describes the relationship among the: </li></ul><ul><li>Temperature </li></ul><ul><li>Volume </li></ul><ul><li>Pressure </li></ul><ul><li>If the number of particles of a gas are constant </li></ul>