ADMS 3530 : 2006.pdf

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cyanskunk957

1 Jun 2014

School

York University

Department

Administrative Studies

Course

ADMS 3530

Professor

Lois King

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Document Summary

Section _____ id # ______________________ (prof. king"s section a; prof. kohen"s sections d and g; prof. tahani"s sections c, e and f; This exam consists of 30 multiple choice questions and carries a total of 100 points. Choose the response which best answers each question. Circle your answers below, and fill in your answers on the bubble sheet. Only the bubble sheet is used to determine your exam score. Read the questions carefully and use your time efficiently. The 20 numerical questions are worth 4 points each. The 10 conceptual questions are worth 2 points each. Choose the answers that are closest to yours, because of possible rounding. Keep at least 4 decimal places for dollar amounts in your calculations, and at least 6 decimal places for interest rates. Bonds pay semi-annual coupons unless otherwise stated and have a face value (or par value) of ,000. You may use the back of the exam paper as your scrap paper.

Related Questions

A. COMPLETE THE ANSWER SHEET: write your name, banner id # and the date in the spaces provided on the scantron. All answers must be on the scantron and this exam. B. Read each item carefully; select the word, phrase or expression that best completes the test item. Indicate the answer blackening the appropriate space on your answer sheet. You MUST erase completely to receive credit for an erased item. This AND the scantron must be turned in. All questions are worth 5 points. R = 0.08206 (atm middot L)/(mol middot K) = 8.314 J/(mol middot K) pH = - log[H_3 O^+] pH + pOH = 14 = pK_a + pK_b [OH^-][H_3 O^+] = 10^-14 = K_a times k_b (at least in water, at 25 degree C) pH = pKa + log([base]/[acid]) poH = pK_b + log ([acidy]/[base]) K_p = K_c(RT)^da For a salt that dissociated into a cation with a coefficient of n and an anion with a coefficient of m: Molar Solubility = squareroot K_/n^m^x = - b plusminus squareroot b^2 - 4ac/2a where 0 = ax^2 + bx + c Which of the following solutions would have the second lowest pH? Assume all their concentrations are 0.10 M at 25 degree C. The acid is followed by its K_a value. A) HF, 3.5 times 10^-4 B) HCN, 4.9 times 10^-10 C) HNO_2, 4.6 times 10^-4 D) HCHO_2, 1.8 times 10^-4 E) HClO_2 1.1 times 10^-2 Which of the following are false about systems at equilibrium? A) The rate of the forward and reverse reactions are the same. B) The concentrations of each component are equal. C) The concentrations of each component don't change over time. D Catalysts do not affect the equilibrium. E) This symbol is used in a reaction where an equilibrium is present: - The reaction below has a K_c value of 3.64 times 10^-3. What is the value of K_p for this reaction at 25 degree C? CO_2 (g) C(s, graphite) = 2 CO(g) A) 3.64 times 10^-3 B) 6.09 times 10^-6 C) 8.90 times 10^-2 D) 1.49 times 10^-4 E) 2.17 Express the equilibrium constant K for the reaction in question 3. A) [CO(g)]/[CO_2(g)][C(s)] B) [CO(g)]/[CO_2(g)] C) [CO(g)]^2/[CO_2(g)] [C(s)] D) [CO_2(g)]^2 E) [CO(g)]^2/[CO_2(g)]

ADMS 3530 : 2006.pdf

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