This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: Test Form B3 Name _________________________ Chemistry 112 Section ____________ FINAL EXAM Total Points = 204 TA ___________________________ Monday, 1:00 PM May 4, 2009 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 section number on the answer sheet. Please use all four digits, 0101, 0102, 0201, etc. This is also very important! 6. CODE the test number shown in the upper right-hand corner of this page onto the answer sheet in the block labeled “Test Form” under the Date line at the top right-hand side. This is Test Form B3. 7. Put all calculations on the examination pages. DO NOT PUT ANY EXTRA MARKS ON THE COMPUTER ANSWER SHEET! 8. This exam consists of 60 multiple-choice questions worth 3.4 points each plus a BONUS question worth 3.4 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 17 pages plus a Periodic Table. Please check to be sure that you have them all! Useful Information : 1 atm = 14.7 psi = 101.325 kPa = 760 torr STP: 0ºC; 1 atm R = 0.082 L·atm/K·mol K = ºC + 273.15 YOU MUST TURN IN ALL PAPERS… YOUR EXAM BOOKLET AND YOUR SCAN SHEET TO YOUR TA BEFORE LEAVING THE EXAMINATION AREA! 112 − Final Exam (Test B3) − 05/04/09 KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 2 _____ 1. Flask A contains O 2 (molar mass = 32.0 g mol − 1 ) at a pressure of 200 torr. Flask B, which is identical to flask A in volume, contains twice as many molecules of natural gas CH 4 (molar mass = 16.0 g mol − 1 ) as the molecules of O 2 in flask A. The temperatures of the gases are identical. The pressure in flask B is (a) 100 torr (b) 200 torr (c) 400 torr (d) 600 torr (e) 800 torr _____ 2. At 65 ° C and 500. torr, the mass of 3.21 L of an unknown gas is 3.5 g. The molar mass of this gas is: (a) 21 g mol − 1 (b) 24 g mol − 1 (c) 41 g mol − 1 (d) 46 g mol − 1 (e) 130 g mol − 1 _____ 3. Which of the following gases has the highest density at STP? (a) Cl 2 (b) H 2 (c) SO 2 (d) NO 2 (e) N 2 O _____ 4. What is the density of CO 2 at 25 ° C and 0.954 atm? (a) 0.172 g L − 1 (b) 1.72 g L − 1 (c) 2.04 g L − 1 (d) 0.985 g L − 1 (e) 1.52 g L − 1 _____ 5. How many liters of NO 2 at STP can be produced from the reaction of 25.0 g of Cu with nitric acid?...
View Full Document
This note was uploaded on 04/03/2011 for the course CHEM 112 taught by Professor Harwood during the Spring '11 term at Purdue.
- Spring '11