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RelativeResourceManager3 - CHEM 6B PRACTICE EXAM 3-2(Prof...

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Chem 6B Practice Exam 3-2 1 Prof. Crowell CHEM 6B PRACTICE EXAM 3-2 (Prof. Crowell) Spr 2010 May 17, 2010 *** FILL IN YOUR STUDENT ID NUMBER , NAME , and TEST FORM = B *** Bubble in the correct response on scantron (25 questions, worth 4 pts each) 1. Given the equilibrium constants for reactions 1 and 2 below at 450K, calculate the equilibrium constant for reaction 3 at this same temperature: Rxn 1: N 2 O 5 (g) 2 NO 2 (g) + ½ O 2 (g), K 1 = 3.3 x 10 4 . Rxn 2: 2 NO (g) + O 2 (g) 2 NO 2 (g), K 2 = 6.4 x 10 3 . Rxn 3: 4 NO (g) + 3 O 2 (g) 2 N 2 O 5 (g), K 3 = ?? a) 5.16 b) 26.6 c) 0.5 d) 0.51 e) 0.038 2. At 2000 C, K p = 0.01 for the reaction N 2 (g) + O 2 (g) 2 NO (g). Predict how the concentrations will change to reach equilibrium at 2000 C if 0.4 moles of N 2 , 0.1 moles of O 2 , and 0.08 moles of NO are placed in a 1.0 L container. a) The concentrations of NO, N 2 and O 2 will remain unchanged. b) The concentration of NO will increase; the concentrations of N 2 and O 2 will decrease. c) The concentration of NO will decrease; the concentrations of N 2 and O 2 will remain unchanged. d) The concentration of NO will decrease; the concentrations of N 2 and O 2 will increase. e) The concentrations of NO, N 2 and O 2 will all increase. 3. Consider the following reaction (assume an ideal gas mixture): 2 NOBr (g) 2 NO (g) + Br 2 (g) A 1.0 L vessel was initially filled with pure NOBr, at a pressure of 5.0 bar, at 300K. After equilibrium was established, the partial pressure of NOBr was 3.5 bar. What is K p for this reaction?
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Chem 6B Practice Exam 3-2 2 Prof. Crowell
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