1. Gas Laws Chemistry Mrs. Coyle

2. Factors Affecting Gas Pressure Number of Moles (Amount of gas) –As the number of particles increases, the number of collisions with the container wall increases. Volume –The smaller the volume, the greater the pressure exerted on the container. Temperature –As temperature increases, kinetic energy increases, increasing the frequency of collision. Thus pressure increase.

3. If Mass and Temp are Constant

4. If Mass and Pressure are Constant

5. Boyle’s Law P 1 V 1 =P 2 V 2 T constant # moles constant P vs V hyperbola P V Isotherm High Temp

6. Charles Law V 1 = V 2 P constant T 1 T 2 # Moles constant V T (K) Isobar

7. Guy-Lussac P 1 = P 2 V constant T 1 T 2 # moles Constant isochoric P T

8. Combined Gas Law P 1 V 1 = P 2 V 2_ T 1 T 2

9. Ideal Gas Law: P V = n R T P = pressure Pa = N/m 2 V = volume measured in m 3 n =# of moles T = temperature K R=Universal gas constant =8.314 kPa L / (mol K) =0.0821 L atm/(mol K) =62.3 mmHg L/(mol K)

10. Dalton’s Law of Partial Pressures P tot =P 1 +P 2 +…. Total pressure of a mixture of gases in a container is the sum of the individual pressures (partial pressures) of each gas, as if each took up the total space alone. http://www.wwnorton.com/college/chemistr y/gilbert/tutorials/interface.asp?chapter=ch apter_08&folder=daltons_lawhttp://www.wwnorton.com/college/chemistr y/gilbert/tutorials/interface.asp?chapter=ch apter_08&folder=daltons_law

11. Ideal Gas Laws mostly hold at: Low pressure High temperature