CHEM 001B Lecture Notes - Lecture 8: Kinetic Theory Of Gases, Torr, Partial Pressure
Document Summary
Chem 001b lecture 8: chapter 6. 8 - 6. 9. At 25 , a 1. 0 l flask contains 0. 030 mol of nitrogen, 150. 0 mg of oxygen, and 4 x 10 21 molecules of ammonia. Calculate the partial pressure and mole fraction of each gas. Nh 3 = (4. 21 x 10 21 molecules) ( N total = 0. 030 + 0. 00469 + 0. 00664 = 0. 0413 mol. 2 kclo 3 (s) 2 kcl (s) + 3 o 2 (g) When the water level inside the container matched the water level outside the container the pressure inside p total equals the atmospheric pressure p atm. A sample of kclo 3 is heated and decomposes to produce o 2 gas. The gas is collected by water displacement at 25 . The total volume of the collected gas is. 229 ml at a pressure of 754 torr. V = 229 ml = 0. 229 l. Correct for the partial pressure of water:
