KEY EXAM 1 W2009 PDF - ey .fl Lab Sec. # ; TA: ; Lab...

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Unformatted text preview: ey .fl Lab Sec. # ; TA: ; Lab day/time: Andreas Toupadakis, Ph.D. Winter 2009 CHEMISTRY 2A Section A EXAM 1 Multiple Choice (circle one) Instructions: CLOSED BOOK EXAM! No books, notes, or additional scrap paper m are permitted. All information required is contained on the exam. m Place all work in the space provided. If you require additional space, use the back of the exam. A scientific calculator may be used (if it is a programmable calculator, its memory must be cleared before the exam). (1) Read each question carefully. Exam has 9 pages total. (2) For problems 1-9 and 10-15, there is no partial credit given and only answers marked on this cover page will be graded. (3) The last page contains a periodic table and some useful information. You may remove it for easy access. L9 totalpomts: (4) If you finish early, RECHECK YOUR ANSWERS! 10 b @ . a c e (5) Apply significant figures rules for Part III for credit. 11. a b c d @ 12.abcd 13. a b c®e 14.@b c d e 15. a© c d e #16-17 (16 +12 =28 points) 10-15 total points: Total Score (100) / 100 U.C. Davis is an Honor Institution Possible Points # 1—9 (4 points each) # 10-15 (6 points each) Name Winter 2009 (Page 2 of 9) EXAM 1 Part 1: Multiple Choice, Concepts (4 points each) Select the best answer and enter your choice on the cover sheet — No partial credit 1. By definition, 1 mole is the number of atoms in 12 g of C—12. That number of atoms was found by experiment to be 6.022x1023. This number has: 3 significant figures a. b. 2 significant figures as many significant figures as the number of stars in the sky .0 d. infinite number of significant figures e. 4 significant figures ©AT2009WIN 2. The law of multiple proportions refers to: more than one chemical compound. a chemical compound. a chemical reaction a nuclear reaction a gas ©AT2009WIN {DP-99‘?) 3. Choose the CORRECT formula/name combination. a. A1203 Dialuminum trioxide b. N204 Nitrogen tetroxide HClO Chlorous acid H20 Dihydrogen monoxide 9.0 e. H3N Trihydrogen nitride ©AT2009WIN 4. Choose the CORRECT statement: a. The concept of limiting reactant can also be applied to a reaction with its reactants being in stoichiometric ratio. b. The percent yield is the ratio of the theoretical yield to actual yield. 0. The percent yield is the ratio of the actual to theoretical yield. d. One mole of dreams is 6.02x1023 dreams e. none of the above ©AT2009WlN 5. Which of the following are NOT isomers? a. CH3CH2CH20H and CH3CH(OH)CH3 b. CH3CH2CH2NH2 and CH3CH(NH2)CH3 CH3C(O)CHC12 and CH2ClC(O)CH2Cl CH3NH2 and CH3NHCH3 e. none of the above ©AT2009WIN Name Winter 2009 (Page 3 of 9) EXAM 1 6. Choose the balanced chemical equation for the complete combustion of HOCH2CH20H. a. 2 HOCH2CH20H + 5 02 —’ 3 C02 + 6 H20 b. 2 H0CH2CH2OH + 3 02 ——> 4 CO2 + 6 H20 0. 2 HOCH2CH20H + 5 02 ——> 7 C02 + 6 H20 d. 2 HOCH2CH20H + 5 02 ——> 4 CO2 + 3 H20 e. 2 HOCH2CH2OH + 5 02 —-> 4 CO2 + 6 H2O ©AT2009WIN 7. Arrange the following chemical formulas in order of increasing oxidation number of oxygen: ZnO, K02, 0F2, Na202, 02F2 a. ZnO, K02, Na202, 02F2, 0F2 b. K02, 0F2, Na202, 02F2, Zn0 c. ZnO, K02, 0F2, 02F2, Na202 d. Zn0, Na202, K02, 02F2, 0F2 e. ZnO, 0F2, Na2O2, 02F2, K02 ©AT2009WIN 8. You are buying a bottle of soda with glucose molarity “x” M, and its temperature is 5°C. You forgot to drink it and you did not even open it. The temperature of the day is 25°C. After the solution reaches the temperature of the day, the solution density becomes less and: The quantity of glucose in grams will be less. a. b. The new concentration of glucose will be larger than “x” M. .0 The new concentration of glucose will be smaller than “x” M. d. The volume of the aqueous solution will be smaller. e. The quantity of glucose in moles will be more. ©AT2009W1N 9. The molecular formula for the condensed structural formula of a hydrocarbon below is: a. C 5H8 b. C5H10 c. C 5H12 d. C5H1 1 e. C 5H9 ©AT2009WIN Name 10. 11. Winter 2009 (Page 4 of 9) EXAM 1 Part 11: Multiple Choice, Short Calculations (6 points each) Select the best answer and enter your choice on the cover sheet —- N0 partial credit The cation D3170+ contains: a. 10 protons 10 electrons and 11 neutrons b. 11 protons 10 electrons and 11 neutrons 12 protons 12 electrons and 10 neutrons .0 d. 11 protons 10 electrons and 12 neutrons e. 11 protons 12 electrons and 10 neutrons ©AT2009W1N on‘tomg {VEL/‘rvovtg €€€Civoms 31) 3xL=3 3x¢:3 3x1:3 1'40 £X8l8 ,1x9=°) 1x<a=8 CH 7 3,1 " j— 10 The total amount of oxygen in 1 g of pure water is equivalent to how many molecules of ozone (03)? ©AT2009WIN a. 5x1022 molecules of 03 b. 4x1 022 molecules of 03 c. 3141022 molecules of 03 d. 2x1022 molecules of 03 e. 1x1022 molecules of O3 iWso€ |-\7,0 iwde C01 (lame O; (“a ‘410>( 18.02;) the) LwtoE HLO g woe C03 6.017,)(lO’LzOv, Wo€€(u-€QS> iWo’e O3 ( , 6-01 x 10L3 ws’éQwaS 03 20-1w \O 19.01x3 7/7, "2 1.4,X [O woeeecuveflf O”). 1% Name Winter 2009 (Page 5 of 9) EXAM 1 12. What is the molarity of NaCl if 5.0 g of an 800% pure sample is dissolved giving 500.0 mL of water solution? ©AT2009W1N a. 0.19M . 0.67M b C. 0.73M d 0,29M M-M.(No(€) ':12.CSC5+1§,L‘S T; €8.L{Ll ’03—. e. 0.14M (5.0 (WWCQ)(BOOO '2) Nag 9"”) 1 wo€ NOLCé Pure 2) \OO iwpwé r g8.L\L\ N UVf a, 3/ (6/ <0.§oo L Coeohovx) ' 13. Consider the general chemical equation: 2A + B —> 3 C Assume that you start with 100.0 g of substance A and you eventually isolate 500 g of substance C. If you know that the molar mass of A is 20 g mol'1 and the molar mass of C is 72 g mol'l, find the actual yield, the theoretical yield and the % yield of the reaction that is represented by the above general chemical equation. a. actual yield = 500 g of C, theoretical yield = 500 g, and % yield = 100 b. actual yield = 500 g of C, theoretical yield = 370 g, and % yield = 74 actual yield = 500 g of C, theoretical yield = 640 g, and % yield = 78 d. actual yield = 500 g of C, theoretical yield = 540 g, and % yield = 93 e. actual yield = 100 g of C, theoretical yield = 540 g, and % yield = 19 ©AT2009WIN Adv-mag yieéd MN. (M : 20 awe " MM. Cc) —. 11 Owe .0 -—s ) ‘Theovdccofl yieéé is: 4 ClOO~OaA3<QOD A aE‘lWo‘eA)( {L veto/6C ‘ H a “Fl/leer x/(€€d@ % weed : Adm”? X100: “906C warping C/t ) “Tl/tech I gl—(o a Q Name Winter 2009 (Page 6 of 9) EXAM 1 14. Which of the following samples contains the greatest number of atoms? 5 g of H2 5 g of O 5 g of Oz 5 g Of 03 5 g of C12 ©AT2009WIN 99-99797 5650 S301. 5303 / g3 iii/'5 ZNEL CHOU/IQ [H1 zqqg 15. If your car is 5.00 metric tons. About how many times more massive is your car than a water molecule? a. 107times b. 1029times c. 1014times d. 1067times e. 1034 times ©AT2009WIN Cow :Cgoo meme ioms>(lo E) ‘0 3 t 5.00 'xlO {L «(roux 1 \(a a ' G Cow 3900 MD a (M \eoz a mo H 109 “0'”: G-ED’ZJJUOLg l—\’LO mo—Qecuézs I ’3- H1Owofi-ecweg _ ‘22 \‘\10 ‘1 1.550 MO 3 (8} 6 7,0) S'.OOX\O _ fl \mflcwl : -gé/ (Q, wém): \O W‘UHO) (6) vaH10) 1-6563)‘\O /a/ Name Winter 2009 (Page 7 of 9) EXAM 1 Part III (28 points) Please show all work for calculations — Partial credit may be given 16. (16 points) Calculate the molarity of each type of ion remaining in solution after 50.0 ml of 1.00 M H1 is mixed with 30.0 ml of2.00 M KOH AND 100.0 ml ofwater. Assume all reactants and products except water dissociate completely into ions. ©AT2009WIN (K0.0W€)CQ.OON\ 260.0 vvxvmo—e kOH H1 4- \(<O\-\ “‘9 k1 {- H10 g€£OVC 50-0 “MA/‘06 60.00 \Mw‘og wwoé QMOMSC ~S0.0 <00 J(<00 (VERY 0.0 \0.0 $0.0 ‘l' o. 10.0 wmoe k0“ H 10.0 WWOK K Omcl 10.0 mm on \Mwo’e $0.0 wmoe K+ SOQO wwo’e E- 60.0 ww‘o—e K + O 00 + 650.0 +100 + too. 0) w. e [on -.: NM - 030. 0 we €06“ [1’] : S'O-O mum/C 1' I HBO-O 'wa Name Winter 2009 (Page 8 of 9) EXAM l 17. (12 points) In nature chlorine is found as a mixture of two isotopes. Its atomic % composition has been found to be, Cl-35 (75.77%) and Cl-37 (24.23%). Calculate its mass % composition if you know that the atomic mass of each of its isotopes is: Cl-35 (34.968852 amu) and Cl—37 (36.965903 amu). Hint: atomic % composition and mass % composition are about the same but they are not identical. Use the rules for significant figures solving this problem. ©AT2009WIN r _ . m , . UWCn CHOW/“C, % Cowpocflmomt Cg C€’§€: 4911 (2-35 atom 15111 woé (6’35 N 1.00 C6 glows 100 wo€ CCU Gtvevx OHM/MC wu§§ of C€-%S zq.056‘68§?. owu (‘3 queeesza 01-25 10am cuss me 02-»; Need #0 /€md 2, I CQ'ZS 1003 Cl/VéOVCflQ 194? M w“) imbe a'gg :00 mug imoe C023 > : "FLl*"LLl avzg 39m” 3 cuemme L00 3 cu eovtxn€ 0 00 M 0% Z (proflim‘ow w \0 ’ 7944 ‘fl ’ Name Winter 2009 (Page 9 of 9) EXAM 1 Periodic Table Key Atomic Number 2 Symbol Atomic Mass 4003 Electronegativity . 5 6 7 8 9 10 B C N O F Ne 2.04 2.55 3.04 3.44 3.98 - 13 14 15 16 17 18 AI 5i P 5 Cl Ar‘ 28.09 30.97 32.06 35.45 39.95 1.61 1.90 2.19 2.58 3.16 - 5 r. 3 I 5 Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As 5e B Kr 47.90 50.94 52.00 54.94 55.85 58.93 58.70 63.55 65.38 69.72 72.59 74.92 78.96 79 90 83.80 1.54 1.63 1.66 1.55 1.83 1.88 1.91 1.90 1.65 1.81 2.01 2.18 2.55 2 96 - 4o 41 42 43 44 45 46 47 48 49 5o 51 52 5 54 Zr Nb Mo Tc Ru Rh Pd Ag Cd In 5n Sb Te Xe 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126 9 131.3 1.33 1.6 2.16 1.9 2.2 2.28 2.20 1.93 1.69 1.78 1.96 2.05 2.1 2 66 - 72 73 74 75 76 77 78 79 80 81 82 83 84 8 86 Hf Tu W Re Os Ir‘ Pt Au Hg Tl Pb Bi Po AT Rn 178.5 180.9 183.9 18 .2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (209) (210) (222) 1.3 1.5 2.36 1.9 2.2 2.20 2.28 2.54 2.00 2.04 2.33 2.02 2.0 2.2 - 104 105 106 107 109 Unq Unp Unh Uns Une Some useful equations and data: PLEASE NOTE: Important values and equations required for calculations are given with the respective problem. The following may or may not be of any use. Moles Actual Yield NA = 6. 022 x 10 23 Molarity = __ % Yield = —————— x100 d _ fl — V Volume Theoretical Yield 1 metric tan is 1000 kg 1 lb = 453.59 g I g = 6.022 x 10 23 amu ...
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KEY EXAM 1 W2009 PDF - ey .fl Lab Sec. # ; TA: ; Lab...

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