2006 Academic Challenge

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1 2006 Academic Challenge CHEMISTRY TEST - STATE FINALS This Test Consists of 40 Questions Chemistry Test Production Team Don DeCoste, University of Illinois at Urbana - Champaign Author/Team Coordinator Gretchen Adams, University of Illinois at Urbana - Champaign Author Nancy Carter Dopke, Mercer University Reviewer Don Wayman, WYSE Coordinator of Test Production GENERAL DIRECTIONS Please read the following instructions carefully. This is a timed test; any instructions from the test supervisor should be followed promptly. The test supervisor will give instructions for filling in any necessary information on the answer sheet. Be sure you understand and correctly follow these instructions. You are to indicate your answer to each question by marking an oval that corresponds to the correct answer for that question. Only one oval should be marked to answer each question. Multiple ovals will automatically be graded as an incorrect answer. Be sure ovals are marked as. Not as,,, etc. If you wish to change an answer, erase your first mark completely before marking your new choice. You are advised to use your time effectively and to work as rapidly as you can without losing accuracy. Do not waste your time on questions that are too difficult for you. Go on to the other questions and come back to the difficult ones later if you can. *** TIME: 40 MINUTES *** DO NOT OPEN TEST BOOKLET UNTIL YOU ARE TOLD TO DO SO! 2006 Worldwide Youth in Science and Engineering WYSE, Worldwide Youth in Science and Engineering and the WYSE Design are service marks of and this work is Copyright 2006 Board of Trustees of the University of Illinois at Urbana - Champaign. All rights reserved

2 Periodic Table of the Elements *Lanthanides **Actinides 1A 2A 3A 4A 5A 6A 7A 8A 19 K Ca Rb Sr Cs Ba Li Be Na Mg H Fr (223) 88 Ra Sc Ti V Cr Mn Fe Co Ni Cu Zn Y Zr Nb Mo Tc (98) 44 Ru Rh Pd Ag Cd La* Hf Ta W Re Os Ir Pt Au Hg Unq 105 Unp 106 Unh 107 Uns 108 Uno 109 Une 89 Ac** (227) 31 Ga In Tl B Al Ge Sn Pb C Si As Sb Bi N P Se Te Po (209) 8 O S Br I At (210) 9 F Cl He Kr Xe Rn (222) 10 Ne Ar Ce Pr Nd Pm (145) 62 Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa (231) 92 U Np (237) 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260)

3 The information on this page may be useful in completing this exam. ph = -log[h + ] poh = -log[oh - ] K w = 1 x PV = nrt (R = L atm mol -1 K -1 ) (R = J mol -1 K -1 ) K = C ΔG = ΔH TΔS N A = x atoms mol -1 Assume gases behave ideally unless specifically told otherwise. Assume solutions are aqueous and at 25 C unless specifically told otherwise. STANDARD REDUCTION POTENTIALS (298 K) ε (V) Cl 2 + 2e - 2Cl Br 2 + 2e - 2Br Ag + + e - Ag 0.80 I 2 + 2e - 2I Cu e - Cu H + + 2e - H Al e - Al Mg e - Mg Na + + e - Na K + + e - K Faraday s constant (F) = 96,485 C/mol

4 WYSE Academic Challenge Chemistry Test (State Finals) A 20.0-g sample of a gaseous hydrocarbon (a compound consisting of only carbon and hydrogen) is placed in a balloon at 1.00 atm and 25 C. The volume of the balloon is 16.3 L. The 20.0-g sample of this compound contains 16.0 g carbon. Determine the molecular formula for this compound. a) CH 3 b) CH 4 c) C 3 H 8 d) C 3 H 9 e) C 2 H 6 2. Consider the reaction as represented by the following unbalanced chemical equation N 2 + H 2 NH 3 In which of the following cases is nitrogen the limiting reactant? a) Reacting 60.0 g of N 2 with 10.0 g of H 2. b) Reacting 2.0 moles of N 2 with 5.0 moles of H 2. c) Reacting g of N 2 with 60.0 g of H 2. d) Reacting 3.0 moles of N 2 with 3.0 moles of H 2. e) Nitrogen is not limiting in any of the cases above. 3. Which of the following has the highest ionization energy? a) Mg b) Mg + c) Mg 2+ d) Mg 3+ e) all the same 4. Which of the following is the most ideal gas at room conditions? a) CO b) H 2 O c) HF d) NH 3 e) N 2 5. The electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 is the correct electron configuration for the most stable form of which ion? a) The calcium ion. b) The argon ion. c) The magnesium ion. d) The fluoride ion. e) The oxide ion. 6. Consider a steel container filled with 40.0 g of helium gas (He) and 40.0 g of argon gas (Ar). What is the ratio of pressures that each gas exerts (answers are for He:Ar)? a) 1:1 b) 10:1 c) 1:10 d) 9:1 e) Need more information.

5 Chemistry 2 7. The unit cell in this two-dimensional crystal contains Xs and Os. X X X X O O O O X X X X O O O O X X X X O O O O a) 1,4 b) 2,1 c) 1,2 d) 4,1 e) 1,1 8. Consider a reaction represented by the following balanced equation 2A + 3B C + 4D You find that it requires equal masses of A and B so that there are no reactants left over. Which of the following is true? a) The molar mass of A must be greater than molar mass of B. b) The molar mass of A must be less than molar mass of B. c) The molar mass of A must be the same as molar mass of B. d) More information is needed to answer this question. e) None of the above choices (a-d) are true. 9. You carry out the reaction represented by the following balanced equation N 2 (g) + 3H 2 (g) 2NH 3 (g) You add an equal number of moles of nitrogen and hydrogen gases in a balloon. The volume of the balloon is 1.00 L before any reaction occurs. Determine the volume of the balloon after the reaction is complete. a) L b) L c) 1.00 L d) 1.50 L e) 3.00 L 10. Which of the following are isomers? a) dimethyl ether and ethanol b) propanol and propanal c) ethanol and propanol d) propanone and propanol e) dimethyl ether and methanol 11. Calculate the density of neon gas (Ne) at 1.00 atm and 25.0 C. a) g/l b) 9.84 g/l c) 20.2 g/l d) 22.4 g/l e) None of these.

6 Chemistry Which of the following is the most polar bond? a) C-H b) N-O c) C-O d) O-O e) O-S 13. Consider the reaction between 50.0 ml of M NaOH and 75.0 ml of M HCl. Which of the following statements is true? a) After the reaction, the concentration of Na + is greater than the concentration of OH -. b) The NaOH was the limiting reactant. c) After the reaction, the concentration of Na + is equal to the concentration of Cl -. d) After the reaction, the concentration of Na + is still M because Na + is a spectator ion. e) None of these are correct. 14. Which of the following has the lowest boiling point? a) H 2 O b) C 2 H 6 c) NH 3 d) CH 3 OH e) CH Which of the following molecules is non-polar even though it has polar bonds? a) Cl 2 O b) NH 3 c) CO d) N 2 e) BF Consider separate gram samples of each of the following: NH 3, N 2 O, N 2 H 4, HCN, HNO 3. Which of the samples has the largest mass of nitrogen? a) NH 3 b) N 2 O c) HCN d) N 2 H 4 e) HNO Which of the following gives the correct orders for increasing (from smallest to largest) atomic radius and ionization energy, respectively? a) S, O, F and F, O, S b) F, S, O and O, S, F c) S, F, O and S, F, O d) F, O, S and S, O, F e) none of these 18. You are asked to determine the perimeter of the cover of your textbook. You measure the length as cm and the width as cm. How many significant figures should you report for the perimeter? a) 1 b) 2 c) 3 d) 4 e) Which of the following correctly ranks the atoms from the least electronegative to the most electronegative? a) Li, B, C, N, Na b) K, Na, S, Cl, F c) Fr, N, P, O, F d) Be, Mg, Ca, Sr, Cs e) At least two of the above (a-d) correctly ranks the atoms from the least electronegative to the most electronegative.

7 20. Arrange the following 0.10 M aqueous solutions from lowest to highest ph. Chemistry 4 Kb for NH 3 = 1.8 x 10-5 Ka for HC 2 H 3 O 2 = 1.8 x 10-5 Ka for HF = 7.2 x 10-4 NaOH, HCl, NaCl, NaC 2 H 3 O 2, NH 4 F, NH 3 a) HCl, NH 4 F, NaCl, NaC 2 H 3 O 2, NaOH, NH 3 b) HCl, NaCl, NH 4 F, NH 3, NaC 2 H 3 O 2, NaOH c) HCl, NH 4 F, NaCl, NaC 2 H 3 O 2, NH 3, NaOH d) HCl, NaCl, NH 4 F, NaC 2 H 3 O 2, NH 3, NaOH e) HCl, NaCl, NaC 2 H 3 O 2, NH 3, NH 4 F, NaOH 21. What is the percent oxygen by mass in sodium sulfate? a) 38.1% b) 45.1% c) 49.6% d) 53.8% e) none of these 22. Determine the [C 6 H 6 O 6 2- ] for ml of a M solution of H 2 C 6 H 6 O 6 (Ka 1 = 7.9 x 10-5, Ka 2 = 1.6 x ). a) 4.0 x 10-3 M b) 1.3 x 10-3 M c) 7.9 x 10-5 M d) 1.6 x M e) none of these 23. The vinegar you buy in the grocery store is 0.83 M acetic acid (HC 2 H 3 O 2, Ka = 1.8 x 10-5 ). What concentration of HF (Ka = 7.2 x 10-4 ) has the same ph as vinegar? a) 1.5 x 10-5 M b) 3.9 x 10-3 M c) M d) 0.83 M e) 33 M 24. True or false: The species Cl - is not a good base in aqueous solution. a) True. This is because Cl - is the conjugate base of a weak acid. b) False. The species Cl - is a good base in aqueous solution because it is the conjugate base of a strong acid. c) True. This is because Cl - is a good proton donor. d) False. The species Cl - is a good base in aqueous solution because of its high electronegativity. e) True. This is because water has a stronger attraction for protons than does Cl -.

8 25. Which of the following will raise the ph of a weak acid HA in aqueous solution? I. Addition of water. II. Addition of NaA (s) III. Addition of NaCl (s). IV. Addition of HNO 3. V. Addition of KOH. a) IV only b) II, V c) I, III, V d) I, II, V e) II, III, V Chemistry You add an excess of solid PbCl 2 to water (K sp for PbCl 2 = 1.6 x 10-5 ). Calculate the concentration of Cl - at equilibrium. a) M b) M c) M d) M e) none of these 27. Which of the following has the lowest vapor pressure at a given temperature? a) CH 3 OCH 3 b) CH 3 CH 2 OH c) CH 3 CH 2 CH 3 d) CH 3 CH 2 CH 2 CH 3 e) H 2 O 28. For which of the following is ΔS expected to be negative? a) Table salt dissolves in water. b) N 2 (g) + 3H 2 (g) 2NH 3 (g) c) 2KClO 3 (s) 2KCl(s) + 3O 2 (g) d) Water evaporates. e) ΔS can never be negative. 29. At constant pressure what does a large negative value of ΔG for a reaction indicate? a) The reaction lies further on the product side and occurs more quickly than a reaction with a lower value of ΔG. b) The reaction lies further on the reactant side and occurs more quickly than a reaction with a lower value of ΔG. c) The reaction lies further on the product side but we know nothing of the rates of reaction. d) The reaction lies further on the reactant side but we know nothing of the rates of reaction. e) The reaction lies further on the reactant side and occurs more slowly than a reaction with a lower value of ΔG.

9 Chemistry The experimental rate law for the decomposition of nitrous oxide (N 2 O) to N 2 and O 2 is rate = k[n 2 O] 2. Two mechanisms are proposed: I. N 2 O N 2 + O N 2 O + O N 2 + O 2 II. 2N 2 O N 4 O 2 N 4 O 2 2N 2 + O 2 Which of the following could be a correct mechanism? a) Mechanism I with the first step as the rate-determining step. b) Mechanism I with the second step as the rate-determining step as long as the first step is a fast equilibrium step. c) Mechanism II with the second step as the rate-determining step if the first step is a fast equilibrium step. d) None of the choices (a-c) could be correct. e) At least two of the above choices (a-c) could be correct. 31. The name of the compound PbO 2 is a) lead(ii) oxide b) lead dioxide c) lead oxide d) lead(iv) oxide e) lead oxalate 32. Which of the following is the strongest oxidizing agent? a) Cl 2 b) K c) Cl - d) K + e) H Electrolysis of a molten salt with the formula MCl, using a current of 3.86 amp for 16.2 min, deposits 1.52 g of metal. Identify the metal. a) Li b) Na c) K d) Rb e) Ca 34. You have a system at equilibrium governed by the equation PCl 5 (g) PCl 3 (g) + Cl 2 (g), for which ΔH = -89kJ. How many of the following will shift equilibrium to the right? I. Add more PCl 5 II. Decrease the pressure by increasing the volume III. Remove Cl 2 IV. Decrease the temperature. a) 0 b) 1 c) 2 d) 3 e) A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is element X? a) C b) He c) F d) S e) none of these

10 Chemistry Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is raised? a) The equilibrium position is shifted to the right and the value for K increases. b) The equilibrium position is shifted to the left and the value for K decreases. c) The equilibrium position is shifted to the right and the value for K decreases. d) The equilibrium position is shifted to the left and the value for K increases. e) The equilibrium position is shifted but the value for K stays constant. 37. Calculate the solubility of Ag 2 CrO 4. The K sp for Ag 2 CrO 4 is 9.0 x a) 9.0 x M b) 2.1 x 10-4 M c) 6.5 x 10-5 M d) 3.0 x 10-6 M e) 1.3 x 10-4 M 38. Which of the following is a not a chemical change? a) Adding an acid to a base. b) Adding water to sodium. c) A phase change. d) The oxidation of iron. e) All of the above are chemical changes. 39. Arrange the following forms of electromagnetic radiation from shortest to longest wavelength. a) ultraviolet, infrared, microwaves, blue (visible), red (visible) b) red (visible), blue (visible), microwaves, infrared, ultraviolet c) microwaves, infrared, red (visible), blue (visible), ultraviolet d) ultraviolet, blue (visible), red (visible), infrared, microwaves e) microwaves, ultraviolet, infrared, red (visible), blue (visible) 40. Which organic functional group is represented in the generic formula R-OH? a) amine b) secondary alcohol c) aldehyde d) primary alcohol e) ketone

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