1. Unit 4 Chapter 10 AP Chemistry

2. Unlike liquids and solids, they Expand to fill their containers. Are highly compressible. Have extremely low densities. Volumes are proportional so can be used as mole values when comparing amounts. CHARACTERISTICS OF GASES

3. PRESSURE Pressure is the amount of force applied to an area. Atmospheric pressure is the weight of air per unit of area. P = FAFA

4. Gas pressure is caused by collisions of molecules with the side of the container and other molecules. Pascals 1 Pa = 1 N/m 2 Bar 1 bar = 10 5 Pa = 100 kPa UNITS OF PRESSURE

6. mm Hg or torr These units are literally the difference in the heights measured in mm ( h ) of two connected columns of mercury. Atmosphere  1.00 atm = 760 torr

7. Normal atmospheric pressure at sea level. STANDARD PRESSURE It is equal to  1.00 atm  760 torr (760 mm Hg)  101.325 kPa

8. Used to measure atmospheric pressure More air pressure results in higher level of Hg supported (warm, dry days) Less air pressure results in lower level of Hg supported (stormy, unstable air) BAROMETER

10. For a barometer, shape doesn’t matter, only height.

11. Used to measure the difference in pressure between atmospheric pressure and that of a gas in a vessel. MANOMETER

14. BOYLE’S LAW The volume of a fixed quantity of gas at constant temperature is inversely proportional to the pressure. P 1 V 1 = P 2 V 2

15. AS P AND V ARE INVERSELY PROPORTIONAL A plot of V versus P results in a curve. Since V = k (1/P) This means a plot of V versus 1/P will be a straight line. PV = k

17. CHARLES’S LAW The volume of a fixed amount of gas at constant pressure is directly proportional to its absolute temperature. T = Kelvin (absolute scale) K = Celsius + 273 A plot of V versus T will be a straight line. i.e., VTVT = k V 1 = V 2 T 1 T 2

19. TEMPERATURE & PRESSURE Boyle’s Law P 1 V 1 = P 2 V 2 Charles’ Law V 1 = V 2 T 1 T 2 Combined Gas Law P 1 V 1 = P 2 V 2 T 1 T 2

20. AVOGADRO’S LAW The volume of a gas at constant temperature and pressure is directly proportional to the number of moles of the gas. Mathematically, this means V = kn V 1 = V 2 n 1 n 2

21. V  1/P (Boyle’s law) V  T (Charles’s law) V  n (Avogadro’s law) IDEAL-GAS EQUATION So far we’ve seen that Combining these, we get V V  nT P

22. IDEAL-GAS EQUATION PV = nRT Pressure in atmospheres or kPa Volume in Liters moles Universal gas constant 0.08206 L ·atm K·mole Temp in Kelvin 8.31 L ·kPa K·mole