chem 112 final exam - Test Form B3 Name Chemistry 112...

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Unformatted text preview: Test Form B3 Name Chemistry 112 Section FINAL EXAM Total Points = 204 TA Monday, 1:00 PM Ma. 4.20.09. _ ._ 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. go_Dg your name on the answer sheet using an ordinary (#2) pencil. 4. CODE your correct IO—digit identification number (PUID) on the answer sheet. THIS IS VERY IMPORTANT! 5. CODE your section number on the answer sheet. Please use all Log; digits, 0101, 0102, 0201, etc. This is also very important! 6. CODE the test number shown in the upper rightuhand 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 % 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: latm = 14.7 psi = 101.325 kPa = 760 torr STP: 0°C; 1 atm R = 0.082 L-atm/K-mol K = °C + 273.15 YOU MUST TURN IN ALL PAPERS... YOUR EXAM BOOKLET AND YOUR SCAN SHEET TO YOUR TA BEFORE LEAVING THE EXANIINATION AREA! 112 - Final Exam (Test B3) - 05/04/09 1. Flask A contains 02 (molar mass = 32.0 g Incl—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 CH4 (molar mass = 16.0 g mol“) as the molecules of 02 in flask A. The temperatures of the gases are identical. The pressure in flask B is ‘ (a) 100 torr .. (b) .. .. 20.0..t9rr. .. . (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 (0) 41 g mol—1 (d) 46 g motl (e) 130 g moi—1 _ 3. Which of the following gases has the highest density at STP? (a) C12 0’) H2 (0) 302 (‘1) N02 (6) N20 4.. What is the density of C02 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 N02 at STP can be produced from the reaction of 25.0 g of Cu with . nitric acid? Cu(s) + 4HN03(aq) —> Cu(N03)2(aq) + 2 H20(fl) + 2N02(g) (a) 44.8 L . (b) 35.2 L (c) 4.41 L (d) 8.82 L (e) 17.6 L KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - Final Exam (Test B3) - 05/04/09 6. How many molecules are in 0.025 mol of H2 gas? (a) 1.5 x 1022 (b) 1.5 x 1023 .. (0.) . -3.-4 19102.3 .. (d) 2.4 x 1023 (e) None of the above 7. When compared to H28, H286, and H2TC, water is found to have the highest boiling point because it: (a) has the lowest molar mass. (b) has the smallest molecules. (0) forms hydrogen bonds. ((1) supports life. (e) forms ice readily. 8. The process by which a solid changes directly to vapor is called: (a) vaporization. (b) sublimation. (c) evaporation. ((1) fusion. (6) condensation. 9. If 5.0 g NaCl are dissolved in 25.0 g of water, the percent ofNaCl by mass is: (a) 0.019% (b) 20.0% (c) 0.20% (d) 17% (e) None of the above 10. How many milliliters of 6.0 M H2804 must one use to prepare 500. mL of 0.20 M sulfuric acid solution? (a) 30 mL (b) 17 mL (0) 12 mL (d) 100 mL (e) 10 mL KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - Final Exam (Test B3) - 05/04/09 11. Calculate the number of calories necessary to convert 30.0 g of ice at its melting point to steam at its boiling point. The specific heat capacity for H2002) = 1.00 cal gw1 °C_'. The heats of fusion and vaporization are 80 cal g"1 and 0.54 kcal g4, respectively. (a) 2.40 x 103 cal . ..(b) kcal... .. (c) 16.2 kcal (d) 21.6 kcal (e) 30 kcal 12. A liquid boils when the: E (a) vapor pressure of the liquid equals the external pressure above the liquid. i (b) heat of vaporization exceeds the vapor pressure. ' (c) vapor pressure of the liquid equals 1 atm. (d) boiling temperature for that liquid is reached. (e) bonds holding the atoms together break. 13. When a solute is dissolved in a solvent: (a) the freezing point of the solution increases. (b) the vapor pressure increases. (c) the boiling point of the solution increases. (d) the concentration of the solvent increases. (6) a chemical reaction occurs. 14. What mass of BaC12 will be required to prepare 200. mL of 0.150 M solution? (a) 0.750 g (b) 156 g (c) 31.2 g (d) 3.12 g (e) 6.25 g 15. When the reaction: A1 + HCI —> is completed, which of the following molecules is a product: (a) HCl (13) H2 (c) A1012 (d) AIHCI (e) 02 KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! l 12 - Final Exam (Test B3) - 05/04/09 16. A solution has an [H30+] = 3.4 x 10'5 mol U1. The pH is: (a) 4.47 (b) 5.53 (c) 3.53 _ .(d). _ ._..5-_47 (e) 9.53 17. What is the pOH of the solution in QuestiOn 16 above? (a) 4.47 (b) 8.47 (c) 9.53 (d) 8.53 (e) O 18. The equilibrium constant equation for the reaction: ‘ 2 A(g) + Med —> 3 0(a) + D(s) IS: (a) [C] [D]/[A] [B] (b) [2A] [B]/[3C] [D] (c) [er/[Ar ((1) Must be determined experimentally (e) [Grim/[Arm] _1 9. In the equilibrium reaction: N2(g) + 02(g) —> 2 N02(g) As the pressure is increased, the amount of N02 formed: (a) increases. (1)) remains the same. (c) decreases. (d) increases initially then decreases. (6) cannot be determined. 20. If HCl(g) is added to a saturated solution of AgCi, the concentration of 1ngr in solution: (a) increases. (b) remains the same. (c) decreases. (d) increases initially then decreases. (e) increases and decreases irregularly. KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - Final Exam (Test B3) — 05/04/09 21. 23. 22. 24. A solution with a H of 5.85 has an H30+ concentration of: P (a) (b) ....(o).. .. .. (d) (e) 7.1 x 10‘5 M 7.1x10‘6 M 318x.10*.‘M... . 1.4x 10‘5M 1.4x10_6M Ice floats on water because: (a) (b) (C) (d) (6) it’s less dense than water. it’s more dense than water. its hydrogen bonding is stronger than water. it loses much of its hydrogen bonding. We do not have a good reason to explain this observation. The equilibrium expression for the water gas shift reaction: is: CH4(g) + H20(g) («—2 CO(g) + snag) (a) K = [COHCHAJ (13) K "—'” [CH4] [H20] (0) K = [CH4][H20] [CO][H2] 3 [CH4][H20] (e) cannot be determined from the balanced chemical equation alone Addition of a Cu catalyst to the equilibrium reaction in question (23) above has the following effect: (a) no effect (b) speeds up the rate of reaction (0) cools the reaction to lower temperature (d) favors formation of products, H2 and CO (6) controls the amount of steam needed for the reaction KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 w Final Exam (Test 133) - 05/04/09 25. 26. 27. 28. What is an oxidation—reduction reaction? (a) An oxidation-reduction reaction is an ionizatiou reaction. (b) An oxidation-reduction reaction is a reaction in which an acid reacts with a base to .‘nll I. II ‘I II‘. II Illnl transferred from an electron donor to an electron acceptor. (d) None of the above. Identify the correct statement to describe the process represented by the equation: NaOH —> Na+ +0H‘ (a) Acid base reaction (b) Redox reaction (0) Nuclear fission reaction (d) Ionization of NaOH in water Identify the correct statements for the following reaction C12 + 2Br" —> 2Cl_ + Br; (i) This is redox a reaction. (ii) This is not a redox reaction. (iii) In the course of that reaction, C1 gains an electron, Br _ loses an electron. (a) (ii) and (iii) (b) (i), (ii), and (iii) (c) (i) and (iii) (d) All three statements are false. To decide whether or not we are dealing with a redox reaction, why do we determine the Oxidation state of the chemical elements before and after a reaction? (a) Because gain of electrons would decrease the oxidation state of an element; loss of electrons would increase its oxidation state. (b) Because gain of electrons would increase the oxidation state of an element; loss of electrons would decrease itsoxidation state. (0) Both (a) and (b) are correct. ((1) Both (a) and (b) are incorrect. KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - Final Exam (Test B3) - 05/04/09 8 29. Consider the following reaction: 4Fe + 302 9 2136203 Which of the following statements correctly describes the oxidation state of iron in that reaction? (b) The oxidation state of Fe changes from 4 to 2+. (0) The oxidation state of Fe changes from 0 to 3+. (d) The oxidation state of Fe does not change. 30. Identify the balanced half-reactions for the following redox reaction: 5 2Fe + 3C12 ——> 2FeCl3 \ (a) 2Fe —> 2Fe3+ + 6e— 3C1; + 6e_—-> 6C1— (b) Fe —> 2Fe3+ C1; —> Fer (0) Fe -> FeCl3 C12 +2e‘ —> 2C1w (d) 2Fe+3e‘—>2Fe3+ Clz+26T—) 31. Identify the nuclear symbol of the Cobalt isotope that contains 32 neutrons (a) 3% Co (b) 39; Co (c) 3% Co (d) None of the above 32. To image Alex's thyroid glands, an endocrinologist gave him pills containing 1-131. 1%1 we lgiXe + 3,6 + yrays Identify the product used by the endocrinologist to image Alex's thyroid glands. (a) Xe— 1 3 1 because it is radioactive (b) 3 fl , because beta particles can penetrate through human tissues (0) 7 rays can penetrate through human tissues and therefore can be detected by a suitable detection system ((1) None of the above KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 — Final Exam (Test 133) W 05/04/09 9 33. 34. 35. 36. (b) ...N9,afavorahle.deca..should. reduce. Is the following mode of decay favorable? l‘gc —+ 1‘.},N + 3,6 (a) No, a favorable decay should produce N—13. 4 (c) Yes. The N/Z ratio in C-14 is 1; beta emission producing N-14 would bring the N/Z ratio to 1.33, which is in the stability range. ((1) Yes. The N/Z ratio in 014 is 1.33; beta emission producing N—l4 would bring the N/Z ratio to 1,which is in the stability range In the following list, identify the correct statements. (i) The rate of radioactive decay is measured by half-life. (ii) Half-life is the time it takes for half of the atoms in any given quantity of a radioactive isotOpe to decay. (iii) Half-life has a characteristic value for each radioisotope. (iv) The unit of half—life is always time. (V) The unit for measuring half-life is Curie. (a) All of the above. (b) None of the above. (c) (i), (ii), (iii), and (iv) ((1) (i), (ii), (iii), and (V) When bombarded by a neutron, U-235 undergoes fission, emitting Sb-133 and Nb-lOO. Determine how many neutrons are emitted in the fission reaction (a) 0 (b) 2 (c) 3 (d) 4 In some cases, nuclei of an unstable atom may capture an electron from the Is orbital of the atom. As the result of electron capture, a proton combines with the captured electron to form a neutron. Identify X, the product of the following electron capture reaction. ZBe + 3}? —> %X (a) ZHe (b) SHe (0) gm (d) in KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - Final Exam (Test B3) - 05/04/09 10 37. Classify the following molecule: NHg—(CH2)4—NH2 (a) Alkene b. .. ...Alcohol. .. .. .. . .. (c) Amide I (d) Amine 38. Identify the following molecules: (a) Two equivalent structure of benzene (b) l ,3 ,4-hexene (0) Two forms of cyclohexane ((1) Two forms of 1,3,4-pentene 39. Name the following molecule: CH3CH2CH20H (a) Methanol (b) Ethanol (c) 1 -butanol (d) l-propanol 40 . Name the following molecule: ' CH3CHCH2CH2CH3 CH3 (a) 2-hexane (b) isobutane (c) pentane (d) 2—methylpentane KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - Final Exam (Test B3) - 05/04/09 11 41. Name the following molecule (a) Pentane (b) Hexane : (c) Octane (d) Butane 42. Name the following molecule: | i (a) Hexane (b) Heptane ; (c) Octane ((1) None of the above. 43. _ Name the following molecule: 1 | CH3 Citizens (a) 5-ethyl-3-methyloctane (b) Butane (c) 4—butyl-6-methyloctane (d) n—octane 44. Name the following molecule: H3C-CH2-CHmCH2 (a) 1-butene (b) 3-butene (c) 1—propene (d) 3-propene KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 — Final Exam (Test B3) — 05/04/09 45. Name the following molecule: (a) Cyclopropane (b) Cyclohexane (c) Cyclobutane (d) Cyclopentane 46. Name the following molecule: H I \ P / MGM CI H (a) trans-1 ,2udichloroethene (b) Propene (c) cis-l,2-dichloroethene (d) trans-1 ,2—dichloropropene 47. Identify the products of the following reaction CH4 + 202 —> (a) HCOOH + H2O (b) CO2 + 2 H20 (0) Propene (d) Hexane 48. Identify the product of the following reaction CH2=CH2 + H0] —> (a) Chloroethane (b) Chloroethene (c) Chloromethane (d) . None of the above KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 12 112 — Final Exam (Test 133) — 05/04/09 13 49. Identify the functional groups in the following molecule: eazmezamoooa "Pitta a” time 'y , anamme, 'a'c'a'r 'ox'y to am 1 (b) an amine and a carboxylic acid (0) an amide and a carboxylic acid (d) None of the above 50. Identify the functional groups in the following molecule: megawatt-sew ea an? (a) An amide, an amine, and a carboxylic acid (b) A methyl, an amine, and a carboxylic acid (0) An alcohol group, an amine, and a carboxylic acid (d) None of the above 51. Classify the following molecule: HsCinCk (C-HflfiDOH - \. w / i /C—C\ H H (a) A saturated fatty acid (b) An unsaturated fatty acids (0) DNA (d) Glycerol 52. Classify the following molecule: ttttttttttttttttto H”? Fl“? 1”" I dd“???iwi“‘i“f“i“f“imc“0fi HHHH" HHHHHHHHHHHH ('3 ('3 {If-#0 (a) alkene (b) alkane (c) saturated fatty acid ((1) unsaturated fatty acids KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 — Final Exam (Test B3) — 05/04/09 14 53. Classify the following molecule: 0 H II HzN—c—Cm-OH ...CH2 . (a) Lipid 1 (b) Saturated fatty acid 1 (c) Glucose (d) Amino acid 54. Identify the functional groups in the following molecule: l a g H3C£H2$)r\ _ /({3H2)7-CB{}H /‘i—C\ H H (a) A double-bond and a carboxylic acid (b) An amine, a double-bond, and a carboxylic acid (0) An alcohol, a double—bond, and a carboxylic acid (d) None of the above. 55. - In the boxed sections, identify the peptide bond fl) (:1) (iii) ‘1? 1? {EBLQ {ail-i3 N H2 (3) (i) (b) (ii) (0) (iii) (d) (iv) KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 - F inal Exam (Test B3) - 05/04/09 56. Which of the following correctly shows the product of the reaction between serine and alanine? {if-{32% {505$ Isiah} ~(g-H + {tigé’émgimi-E W 352?“??th . .....¥‘§s... At flflgi‘fi {jg-fig . 3 H; i itfigN —— N “ii (233;; m3, 3 (3,33%? TB; {gem enga- - H. HEN” .wenr-N—ég—e an; {jg I it i} ii {2- ii . i E! i {E}: the ~£é§ we WERE”? m1 i gag mg {Diff 1?}. nan? 42-4.: min; 2 H E 3:12:41: Ma) mum? m iii? em (a) A (b) B (C) C (d) _ D KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 1 12 7 Final Exam (Test B3) — 05/04/09 16 57. In the following list, identify the correct statements: (i) 0L Helix represents a secondary structure found in proteins. (ii) [3 strand (or [3 sheet) represents a secondary structure found in proteins. (iii) The polypeptide chain in a protein assumes a 3-dimensional structure known as tertiary structure. _ (iv). _ Quaternarystrnsturc corresponds. to the relative arrangement 9f Several __ polypeptide chains in a protein. (a) (i) and (iv) (b) (i) and ((ii) (0) (iii) and (iv) (d) 0), 00,010, and (iv) 58. Shown below is the nucleotide DNA sequence of a short piece of DNA: AGCTTGTTC Which of the following should be written under the sequence to produce the complementary strand? (3) CTTGTTCGA (b) TCGAACAAG (c) CACAACCTC (d) None of the above 59. Classifythe following molecule: AAAAGCUUUUACCCGGGG (a) The sequence of a short piece of DNA. (b) The sequence of a sh0rt peptide. (0) The sequence of a short piece of RNA. ((1) None of the above 60. Identify the following molecule: EEC—OH HO“ OH 32C m OH (a) acetic acid (b) glycerol (0) carbonic acid ((1) ethanol KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 112 — Final Exam (Test 133) — 05/04/09 17 BONUS (3.4 pts.) 61. Identify the products of the following reaction: I EIng ooqmgwws + 3 H20 i ‘ (b) I M— oocgcuaggca-ta 1-K} wows—1930143 + 3 H20 Hzc— (30003-1980013 (0) chw— OOCOCHQEZCHE, 1-K}- ooqcmhzcytg + 3 H20 0130—- 0000;103:0343 (d) ' None of the above KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! 1 12 — Final Exam (Test B3) — 05/04/09 18 ANSWERS ' 35. C 5. E i 6_ A 36. D 7_ C 37. D 8' B 38. A 9. D 39. D 10. B 40. D I u D 41. D _ 12. . A 42' C 13‘ C 43. A 14. E 44. A 15‘ B 45. D 16 A 46. A 17. C 47. B 18. E 48' A 19 B 49. B 20‘ C 50. c .21. E 51. B 22‘ A 52. c 23' D 53. D 24. B 54' A 25. C 55. B 26. D 56. C 27_ C 57. D 28_ A 58. B 29' C 59. C - 30 A 60. B 61. c (BONUS) KEEP YOUR ANSWERS AND WORK COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! ...
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This note was uploaded on 02/27/2012 for the course CHEM 112 taught by Professor Harwood during the Spring '11 term at Purdue University-West Lafayette.

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chem 112 final exam - Test Form B3 Name Chemistry 112...

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