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Unformatted text preview: Test 22 Name _________________________ Chemistry 116-A Section ____________ EXAM II Total Points = 150 TA ___________________________ Wednesday, 8:30 PM March 5, 2008 THIS EXAM IS FOR STUDENTS WITH MONDAY-WEDNESDAY 10:30 or 11:30 LECTURE. YOU SHOULD HAVE AN ORANGE COMPUTER ANSWER SHEET! Directions: 1. Each student is responsible for following directions. Read this page carefully. 2. Write your name and other requested information on this page and on the separate answer sheet. 3. CODE your name on the answer sheet using an ordinary (#2) pencil. 4. CODE your correct 10-digit identification number (PUID) on the answer sheet. THIS IS VERY IMPORTANT! 5. CODE your lab section number on the answer sheet. Please use all four digits, 0101, 0201, 0301, etc. This is also very important! 6. CODE the test number shown in the upper right-hand corner on the answer sheet in the block labeled “Test/Quiz Number”. This is Test 22. 7. Put all calculations on the examination pages. DO NOT PUT ANY EXTRA MARKS ON THE COMPUTER ANSWER SHEET! 8. This exam consists of 20 multiple-choice questions worth 7.5 points each and 1 extra credit question worth 3 points. Choose the one best or correct answer for each question and write it both on your exam paper and on the computer answer sheet. The computer answer sheet is the only one that will be graded! 9. This exam consists of 6 pages plus a Table of Useful Information, a Table of Acid-Base Ionization Constants, a Periodic Table and 2 sheets of scratch paper. Please check to be sure that you have them all! KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK!! 116-A − Exam 2 (Test 22) − 03/05/08 2 _____ 1. Calculate the equilibrium constant, K p , for the following chemical reaction: 2 2 3 2 SO (g) + O (g) 2 SO (g) if the equilibrium partial pressures are 0.15 atm SO 2 , 0.023 atm O 2 , and 0.38 atm SO 3 at 1000 K. (a) 9.1 × 10 −3 (b) 1.1 × 10 2 (c) 2.8 × 10 2 (d) 3.6 × 10 −3 (e) None of the above _____ 2. Which of the following is a true statement about chemical equilibrium in general? Choose the best answer. (a) At equilibrium, the rates of the forward and reverse reactions are equal. (b) At equilibrium, the rate constants of the forward and reverse reactions are equal....
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This note was uploaded on 02/27/2012 for the course CHEM 116 taught by Professor Stevenson during the Spring '08 term at Purdue.
- Spring '08