[Bush] Chemistry Exam #2 - Fall 2007

[Bush] Chemistry Exam #2 - Fall 2007 - NAME 1 Chemistry...

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Unformatted text preview: NAME 1 Chemistry 1301 Fall 2007 Exam #2 PUQfiJIifi PLEASE READ THESE INSTRUCTIONS CAREFULLY BEFORE BEGINNING THIS EXAMINATION. Select the best response to each question. There is only one best response to each question unless otherwise indicated in the question. There are 30 questions in the first part of this examination worth 3.0 points each. The remaining 10 questions on the formulas and names of chemical compounds are worth 1.0 point each. (Total of 100 points.) Check your test booklet to be sure that you have a complete exam with all 40 questions. Write your NAME and TEST NUMBER on your Scantron. Write your name on the first page of the test booklet also. Work each problem carefully on the test booklet or on the scratch paper provided. Then select the answer, which you feel is the best response. If none of the choices is close to your calculated answer, or if none is correct, then select the response "none of the above." ALL ANSWERS MUST APPEAR ON THE SCANTRON. Your grade will be determined only by what appears on the Scantron, not by work on the test booklet. Look over your exam and work the easiest problems first, saving the more difficult ones for last. Be sure that you have correctly indicated your final choices on the Scantron before turning in your paper. If a question is incorrectly marked on the Scantron, it will be counted wrong even if it was correctly marked on the test booklet. If you have any questions about any of the problems on this exam, it is your responsibility to ask for a clarification from the instructor during the examination. —-u_..—__———_——__———.—._—.———._——————__.__—_—_————____.—_—————_——-—n—-...__—————_.— l. A sample containing one mole of each of the following elements is weighed out and placed in separate containers. Which sample contains the most number of atoms? a) Sn b)Pb mmVufifl AuxgdwdSJMSWhek c) Co d) Fe All samples contain the same number of atoms. 2. Avogadro's number is defined as the number of atoms in a) exactly 12.000... g of naturally occurring carbon b) exactly 14.000... g of lag c) exactly 13.000... g of 136C (E9 exactly 12.000... g of 126C e) none of the above .3- 5. Calculate the mass, in grams, of 0.350 mol Cu. a) 18.5 0.350 and Cu 63.550; CL rrxn Cll Calculate the number of Cl atoms in 14.5 g of CCl“ a) 1.42 b) 2.55 X X X X 1022 1025 1022 1023 of the above w\daU-nflflflLb(1:]q;3 f53.55| 93 ’4‘501wt+('m°}ec‘¥ flamerfl Inogfi4kfl 23 l 397%”) Q drum Calculate the mass percent of nitrogen in HNOZ. inoimr‘rmb F4001: 47.0633 Alma-LA Imd U Wmol % HMOlor 14.013 ( reel 941mg) x 100 : $1.830 M e) none of the above (:3 29.8 :- 22.2%04 23 6.02:0qu W Nitrogen and oxygen form an extensive series of at least seven oxides with the general formula Nxoy. One of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of the oxide? a) N20 b) NO C) N02 @ N203 %O: Nieébroééib ’ :44.cn e) none of the above £00.00 seed, = as .Io‘Po O N .—.. O . . E5 "23.00 2% 394 2‘2f5 2.e55 ZKC§OICDLS:)-l }\)1£:)3 7. The empirical formula of the reduced form of lactobionic “ 3 acid, a sugar used in some medicinal agents, is CHZO. The molecular mass of this compound is 360. What is the molecular formula? _ (1mg “WU/me 50-029» s/mo! a) CHZO b) C3H603 300 : use at I; @C12H24012 I BQiOZb d) CsHloOS l1<CH20> : GILHZWOIL e) none of the above 8. What is the mass percent composition of carbon in a 0.100 g sample of a carbon—hydrogen—oxygen compound? The compound, when combusted in oxygen, provided 0.220 g CO2 and 0.239 g water. Q. 60.0 :1 44'0‘ 9 /W\ b) 4.16 oazojflolcrmlgéL WM LOISC : Cloboofic C. I +0191sz «9? ‘ \c “5'5 2%. L CO WW magmas: 60.0%)(1 d) 8.76 (9.100932: e) none of the above 9. When the following equation is balanced using the smallest whole numbers, what is the coefficient in front of H20? Be3N2 +5H20 ~953e(0H)2 +ZNH3 a) l b) 2 c) 3 d) 4 none of the above 10.Suppose that 1.00 mol of each reactant in the following 4 equation is present. Which species is the limiting reagent? mm; + 5AS203 + 9H20 + 12H+ —> 10143124504 + 4Mn2+ a) Mn04 is limiting [(A£U>4QJCHCS$I?YXLAXh/ 10‘ b) Asflh is limiting ‘gb'vflthVN H] c) H20 is limiting @ H is limiting ' e) none are limiting 11. A reaction, which produces crude iron from iron ore, is shown below as a balanced equation: FeZO3 (s) + 3 CO (g) -> 2 Fe (5) + 3 C02 (9) How many moles of iron could be produced from the reaction of 30 mol FeZO3 and 25 mol of CO? a) 60 3cm P2203, m 3 60mm Fe @ 17 ‘mo‘. F27, C) 30 mo zmotpe en —» !7 V F 287nm. .: I . mo. d) 25 ( BmoLCo 8 e) none of the above 12. Calculate the molarity of a solution containing 0.215 mol HF in 825 mL of solution. 7 a) 0.252 M HF o.Q\SrrdHF ‘ 0.24::| HHF b) 2.61 M HF 02251.» 5W" c) 3.84 M HF d 0.215 M HF none of the above 13. What would be the molarity of a solution obtained by diluting 125 mL of 6.00 M HC1 to 500. mL? a) 1.25 M HC1 Haw 1 ytme (g; 1.50 M HC1 _ c) 0.667 M HC1 . Haw: Hm<YELL d) 24.0 M HC1 Vd‘u e) 10.4 M HC1 : (poocndHCJ owZSL} LSOHPQ ha c76EIIDLJ 14. A weak electrolyte is one that _ 5 a) dissolves in water and ionizes completely. b) reacts with water to form hydrogen and oxygen. 10) does not dissolve in water. @ dissolves in water and ionizes to a limited extent. e) precipitates in water. 15. Reduction cannot occur without a) acid b) base 0) water d) air @ oxidation 16. What happens when NaCl and NH3 are dissolved together in water? a) NaOH precipitates no) Lu 561936“) b) NH4C1 precipitates no) chu c7 C12 gas is evolved “ow ocCUIM + @ OH_ is produced L59}; MHz-k HZCD $0141!— 0H4. e) N2 gas is evolved no N (raw 17. What is the concentration of chloride ion in a 0.100 M solution of FeCl3? a) 0.100 M chloride oaooH, Sam3< 39! D: 0mm b) 0.150 M chloride | heel c) 0.200 M chloride @ 0.300 M chloride e) none of the above 18. Zn lies above Pb in the activity series of metals. Which of the following statements is correct? Zn will react with Pb2+. b) Pb2+ will react with Zn2+. c) Zn2+'will react with Pb. d) Pb will react with Zn2+. e) Zn will react with Pb. 19. Which one of the following is a spectator ion in the 6 reaction between NaOH and HCl? V (a Na+ Ma?) + 03-31?) + H2053 +97’Caij’7wcmi3 t/ch/mé ) 4' Hap b) OH— O) H20 d) H+ e) all are spectator ions 20. If you mix aqueous solutions of each of the following, which one will NOT produce a precipitate? a) ngmom + KI Hwa b) Feso4 + Ba(OH)2 FQLOHqux 130.304.? 'c) Pb(NO3)2+ NazCO3 bbcoaJ, d) ZnCl2 + (M1st 2n8\!/ (EE all of the above produce precipitates 2 7C ‘ _ 21. What is the oxidation number of chromium in Cr2072? a) +2 b) +3 ' :zm 762) = —2 2x: 14—2: \7. C) +4 x: +9 @+6 e) none of the above \ .- 22. What is the oxidation number of sulfur in the compound+Naggzozé a) —2 b) +4 20.) +2C>0+5623= o c) +3 1+2x_b:o @ +2 2x:Q;—Z= 4- e) none of the above X = +2 4\ —1 23. What is the oxidation number of oxygen in the compOund Na202? a) +2 b) +1 @ _]_ 2C4b4—2C-1) :D d) -—2 e) none of the above 24. 25. 26. What is the oxidation number of H in molecular hydrogen (H2)? a) —l b) +1 c) +2 d) —2 (g) none of the above 0 In the reaction proceeding in the direction shown below, + 2+ + => + ZAg(aq) Cu(s) Cu (aq) 2Agm) which species is being reduced? (:D‘Ag+( ) fimf ;> Ac, (LKILLLQCQ) aq b) Cum Cu .9 (3.3+ (ULthgaCQ) 2+ c) Cu (aq) d) Ag(s) e) H20 Balance the redox equation below to give the smallest, whole number of reactant and product species. Al + H+ => Al3+ (s) (aq) H2<g> What is the coefficient in front of H2(g) in the correctly balanced equation? 0 +\ *a.&¥ 0 a) l +. 3 b 2 [m_-+3L4 “9’ A4 figul- d) 4 “32, e) none of the above 1“: 3+ RAH- 6H+ ‘4? 2’5“ “Psi—‘2‘ 27. If the correctly balanced equation below were written as 8 a net ionic equation, which species should NOT be shown? (In other words, which species is only a spectator ion?) + BaCO3(S) ZHBr(aq) * => BaBr2(aq) + H20(l) + C02(g) BaCOgs) + 2H 0123 + 2%(953 a +Mcuf) +~ Hz?) w; a) H+(aq) Br_(aq) C) HZO(l) d) Ba2+<aq> e) All of the above should be shown in the net ionic equation. 28. A 1.45 9 sample of an iron ore is dissolved in acid and the iron obtained is Fe“ (aq). To titrate the solution, 21.6 mL of 0.102 M KMnO4 (aq) are required. What is the mass percent of iron in the ore? 2 — 2 5Fe+ + Mno4 + 8H+ 9 5Fe3+ + Mn+ + 4HZO 8-) 57 . 6 o. \OZK\<?(004<°'07—'6 L KHHQB = Z-ZOxldsndQAKHflozp ‘ @42'4 g.a0xlg>ml‘/mnoq(8md Fer 535583 E: = 6.152103% . ‘6 .4 “WNW md (:0, e) 61.5 6" lNoc’ Fe -—————-———, woo,- ,° l.4§g§awfl9’ 414/0 29. Using the Periodic Table, predict the highest and lowest oxidation states for the element 8? a) +7 and —1 (9 +6 and —2 c) +5 and —3 d) +4 and —4 e) something else 30. The following reactions V 9 o 0 'H -r l. 2Na(s) + F2(g) —> 2NaF(s) 2. AgNO3(aq) + KCl(aq) —> AgCl(s) + KNO3(aq) 3. @uaq) + [email protected]) —> H20(l) + KCl(aq) 06:02 LJGQQ, are examples of a) three redox reactions. b) precipitation (first two) and acid—base reactions (third). (g? redox (first), precipitation (second), and acid—base (third). d) three precipitation reactions. e) something else Each one of the following ten questions counts 1.0 point. 31. Cesium ions are expected to have a charge of (E:>+l b) +2 c) +3 «1%)Tfl7 d) —1 q e) —2 32. A correct name for the neutral molecule 803 is a) monosulfur trioxide Cf) sulfur trioxide c) sulfoxide 1‘ d) sulfite mead)! e) sulfate 33. When named as an acid, the correct name for H28 is éfi)hydrosulfuric acid b)hydrosulfurous acid swims Wm 733 c) sulfurous acid d)sulfuric acid e) hydrogen sulfuric acid 10 34. A correct name for the ionic compound NH4CN is a)nitrogen hydrogen cyanate ammonium cyanide c) cyanonitride d)ammonium cyanite e)ammonium cyanate 35. Which one of the following is incorrectly paired? Egi>HCloz = chloric acid C}uoax5<1cico b) HN02 = nitrous acid c) H2C03 = carbonic acid d) H2804 sulfuric acid e) all of the above are correctly paired. 36. Which one of the following is incorrectly paired with its ionic charge? a) hydride ion (—1) b) sulfide ion (—2) c) phosphide ion (—3) d oxide ion (—2) r e) All of the above are correctly paired. 37. Which one of the following is incorrectly paired with its ionic charge? a) oxalate ion (—2) b) thiocyanate ion (—1) c) acetate ion (—1) d) thiosulfate ion (—2) All of- the above are correctly paired. 38. Which one of the following is incorrectly paired? a K2803 = potassium sulfite Co(OH)2 = cobalt(III) hydroxide c) NCl3 = nitrogen trichloride d) NaOCl = sodium hypochlorite e) PtCl4 = platinum(IV) chloride 39. 40. The charge on the ion H803X is: -1 b) —2 c) —3 d) —4 e) none of the above Which metal commonly forms ions with more than one charge? a) Na b) Mg c) Al d) Zn ...
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[Bush] Chemistry Exam #2 - Fall 2007 - NAME 1 Chemistry...

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