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IDEAL gas law

IDEAL gas law. Avogadro (1776-1856) Avogadro’s Hypothesis - any sample of any gas at the same temperature and pressure will contain the same number of particles. The number of moles ( n ) is directly proportional to pressure , and volume. P 1. V 1. P 2. V 2. =. k. n. T 1.

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IDEAL gas law

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  1. IDEAL gas law

  2. Avogadro (1776-1856) Avogadro’s Hypothesis - any sample of anygasat 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. P1 V1 • P2 • V2 = • k n • T1 • T2

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

  5. A steel container with a volume of 20.0 L is filled with nitrogen gas to a final pressure of 2000.0 kPa at 27.00C. How many moles of gas was used? P 2000 V (20.0) = = n R T 27°C + 273 = 300 K L · kPa 8.314 mol · K 16.0 moles n 8.314 (300)

  6. What pressure is exerted by 640.0 g of methane (CH4) gas in a sealed 5.35L container at 27 ºC? 1 mol 16.0 g Molar mass of CH4= 16.0 g/mol (5.35) 640.0 g = 40.0 moles P V n R T = 27°C + 273 = 300 K L · kPa 8.314 mol · K • (40.0) 8.314 (300) 1.9 x 104kPa =

  7. 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 37.00C? 32.0 g 1 mol P 101.3 V (2.2) = = n R T 37°C + 273 = 310 K 0.086 moles 8.314 (310) L · kPa Molar mass of O2= 32.0 g/mol 8.314 mol · K 0.086 mol = 2.75 g of O2

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