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Distributed by the ACS DivCHED Examinations Institute, Iowa State University, Ames, IA. All rights reserved. Printed in U.S.A. 2009 U. S. NATIONAL CHEMISTRY OLYMPIAD LOCAL SECTION EXAM Prepared by the American Chemical Society Olympiad Examinations Task Force OLYMPIAD EXAMINATIONS TASK FORCE Arden P. Zipp, State University of New York , Cortland, NY Chair James Ayers, Mesa State College , Grand Junction, CO Paul Groves, South Pasadena HS , South Pasadena, CA Sherry Berman-Robinson, Consolidated HS , Orland Park, IL (retired) Preston Hays, Glenbrook South HS, Glenbrook, IL Seth Brown, University of Notre Dame, South Bend, IN David Hostage, Taft School , Watertown, CT Peter Demmin, Amherst HS , Amherst, NY (retired) Adele Mouakad, St. John’s School , San Juan, PR Marian Dewane, Centennial HS, Boise, ID Jane Nagurney, Scranton Preparatory School, Scranton, PA Valerie Ferguson, Moore HS , Moore, OK Ronald Ragsdale, University of Utah , Salt Lake City, UT Kimberly Gardner, US Air Force Academy , Colorado Springs, CO DIRECTIONS TO THE EXAMINER This test is designed to be taken with an answer sheet on which the student records his or her responses. All answers are to be marked on that sheet, not written in the booklet. Each student should be provided with an answer sheet and scratch paper, both of which must be turned in with the test booklet at the end of the examination. Local Sections may use an answer sheet of their own choice. The full examination consists of 60 multiple-choice questions representing a fairly wide range of difficulty. Students should be permitted to use non-programmable calculators. A periodic table and other useful information are provided on page two of this exam booklet for student reference. Suggested Time: 60 questions—110 minutes DIRECTIONS TO THE EXAMINEE DO NOT TURN THE PAGE UNTIL DIRECTED TO DO SO. This is a multiple-choice examination with four choices for each question. There is only one correct or best answer to each question. When you select your choice, blacken the corresponding space on the answer sheet with your pencil. Make a heavy full mark, but no stray marks. If you decide to change your answer, be certain to erase your original answer completely.
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Page 2 Not valid for use as a USNCO Local Section Exam after March 31, 2009 ABBREVIATIONS AND SYMBOLS CONSTANTS amount of substance n ampere A atmosphere atm atomic mass unit u atomic molar mass A Avogadro constant N A Celsius temperature °C centi– prefix c coulomb C electromotive force E energy of activation E a enthalpy H entropy S equilibrium constant K Faraday constant F free energy G frequency ν gas constant R gram g hour h joule J kelvin K kilo– prefix k liter L measure of pressure mmHg milli– prefix m molal m molar M molar mass M mole mol Planck’s constant h pressure P rate constant k reaction quotient Q second s speed of light c temperature, K T time t volt V volume V R = 8.314 J·mol –1 ·K –1 R = 0.0821 L·atm·mol –1 ·K –1 1 F = 96,500 C·mol –1 1 F = 96,500 J·V –1 ·mol –1 N A = 6.022 × 10 23 mol –1 h = 6.626 × 10 –34 J·s c = 2.998 × 10 8 m·s –1 0 °C = 273.15 K
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This note was uploaded on 11/30/2010 for the course CHEM 121 taught by Professor Heske during the Spring '08 term at University of Nevada, Las Vegas.

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