1. IDEAL gas law

2. Avogadro (1776-1856) Avogadro’s Hypothesis - any sample of any gas at the same temperature and pressure will contain the same number of particles.

3. The number of moles (n) is directly proportional to pressure, and volume. = P1P1 P2P2 T2T2 T1T1 V1V1 V2V2 k n

5. mol · K Experiments with n, V, P, and T give Ideal gas law: = PV R = experimentally determined ideal gas constant. Value of R depends on the units used for pressure. L · kPa 8.314 L · atm mol · K 0.0821 L · mmHg 62.4 n T kR

6. A steel container with a volume of 20.0 L is filled with nitrogen gas to a final pressure of 2000.0 kPa at 27.0 0 C. How many moles of gas was used? = PV nTR = 2000(20.0) n (300) 8.314 L · kPa mol · K 8.314 27°C + 273 = 300 K 16.0 moles

7. What pressure is exerted by 640.0 g of methane (CH 4 ) gas in a sealed 5.35L container at 27 ºC? 640.0 g 16.0 g 1 mol = 40.0 moles = PVnTR 27°C + 273 = 300 K L · kPa mol · K 8.314 (5.35) (300)8.314 1.9 x 10 4 kPa = Molar mass of CH 4 = 16.0 g/mol (40.0)

8. A child lung capacity is 2.2 L. How many grams of oxygen gas do lungs hold at a pressure of 1.00 atm and a normal body temperature of 37.0 0 C? 0.086 mol 1 mol 32.0 g = 2.75 g of O 2 = PV nTR 37°C + 273 = 310 K L · kPa mol · K 8.314 = 101.3(2.2) (310) 8.314 0.086 moles Molar mass of O 2 = 32.0 g/mol