[Bush] Chemistry Exam #2 - Fall 2006

[Bush] Chemistry Exam #2 - Fall 2006 - NAME 1 Chemistry...

Info iconThis preview shows pages 1–11. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 4
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 6
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 8
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 10
Background image of page 11
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: NAME 1 Chemistry 1301 Fall 2006 Exam #2 PLEASE READ THESE INSTRUCTIONS CAREFULLY BEFORE BEGINNING THIS EXAMINATION. Select the best response to each question. There is only gne 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 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. 1. One mole of each of four elements is weighed out and placed in separate flasks. Which flask contains the most number of atoms? a) Fe para AA cfliuosyafxm3§m¥flfislvgmflbe- b) N ‘c) Ba d) Ag All four flasks contain the same number of atoms. 2. Which one of the above flasks contains the most mass? flVfiOA‘WV1DA ‘3) Fe 555547 b) N I4.cob7 C9 Ba $7.327 3? d) Ag Ky7c£8 e) All four flasks contain the same amount of mass. 3. in grams, of 7.34 mol water. 2 uxiEuLHzo Calculate the mass, a) 10.7 b) 0.408 mdwnmb = 20-00831m04 “34"(‘9008/{210105 c) 25.4 : l8-OW95/md H22) @ 132 7.54. md/ZO< names) :_ :32 9M H20 e) 18 0 nNDL Carbon disulfide, CSZ, can be made from the reaction of graphite and 802. .5..C+_2_-802—>__L<382+fi_co When the equation above is properly balanced with the smallest whole numbers, the respective coefficients are: a 2, 1, 1, 2 (b§>5, 2, 1 4 c) 4,2 1 4 d) 3, 3, l, 2 e) none of the above ‘ I I The very stable compound SF6 is made by burning sulfur in an atmosphere of fluorine. Balance the equation using the smallest whole numbers and then answer the question. 38(8) +2z142(4) ->BSF6<g) If you want to make exactly 2.48 moles of SF6 with no reactants left over, you will need to use at least Ci? 0.310 moles of Sg and 7.44 moles of F2. b) 1.00 moles of Sg and 24.0 moles of F2. c) 0.125 moles of Sg and 3.00 moles of F2. d) 8.00 moles of Sg and 24.0 moles of F2. e) none of the above 3-4ngS/Fe \mdSB 3: o.3\o mo( 88 8mm§Fe Chemical analysis of a compound that contains only oxygen 3 and bromine shows the composition is 58.8% Br and 41.2% 0, by mass . empirical formula of this compound? What is the (Br 79.904 g/mol; O = 15.9994 g/mol). SBE¥§BT<THHTDKVSV ;~ (33755;; yvuzkEBY a) BrO2 :Esjigizg b) Br03 41250 ("mic : 9.578) mot O C) Brzos Okfibv +7 ,S'qm {44> ‘0'12 > “no G e) none of the above A molecule has the empirical formula C4H4O. of of 15. If the molar mass the compound is 272.3 g/mol, what is the molecular formula this compound? (C = 12.011 g/mol; H = 1.0079 g/mol; O = 9994 / 1 g mo ) mm C4040: 402.0") 44(n.oo*z<;)+ 105.9994) “H40 = (98.078 s/mox C8H802 ‘ C H O “172$ : 4 7mth lab) 4 12 12 3 DH C16H1604 4((‘4040‘3 —‘7 C nnH .4904 none of the above Consider the following equation. P4(S) + 502(9) + 6H20(1) ’9 4H3PO4(1) How many moles of the product, H3PO4, can be formed from a mixture in which 1.00 mole of each reactant is present? 100% yield. a 0.800 moles of H3PO4 0.667 moles of H3PO4 AS sume c) 0.500 moles of H3PO4 d) 4.00 mole of H3PO4 \Y\ flag &£L‘ ‘ f th b 9) “one 0 e a We LOO/Ad H10 4% : 0.667 mol é>nvot V4299 t§51¥3k+ 9.Which of the following cannot be an empirical formula? 4 @ CZH2 no+ 5mxb§mm6b J ~ b) CH2 “MW A O smtmwwflo mm m c) CH3 OK d) CZH e) C2H3 10. Using the solubility table attached, predict which one of the following compounds is soluble in water? a) BaSO4 b) HgZCl2 @ Pb(NO3)2 QSLGM‘kcIQO cm 543.96% d) Agzs e) None of the above is water soluble 11. The laboratory has a bottle of 6.00 M sulfuric acid. How many mL of this concentrated solution are required to make 500.0 mL of 0.750 M sulfuric acid solution? a) 36.2 mL of 6.00 M sulfuric acid - 0.5060L(o.750moyt_> 62.5 mL of 6.00 M sulfuric acid VL‘X" _____,_____—————v——'* c) 125 mL of 6.00 M sulfuric acid 6:09 615‘°\/L‘ d) 250. mL of 6.00 M sulfuric acid : 0.0925- L or 625ml- e) none of the above 12. What is the oxidation state of Cl in C120? a) +2 ;- L"'2’ +1 106—240 C) ‘2 21.: Z. d) -—1 x:+, e) none of the above 13. What is the oxidation state of O in 02? a) —2 I b) -1 wwmmfii‘ S56 @ 0 d) +1 e) none of the above X -2 fr- 14. What is the oxidation state of P in KZHPO4? / S a) +1 +[ +3 C) X: 8‘3 3 +3 d) +4 $OG»cm¥3kiQ-—4+up LadeJLgKUJfl>ncmnkn*. @none of the above 15. Which one of the following is a strong acid? a) HNO2 b) HF c) HClO d) H2803 @None of the above is a strong acid. 16. How many grams of NaCl are needed to make 500.0 mL of a 1.50 M solution of NaCl? (molar mass NaCl = 58.4 g/mol) a) 175 grams of NaCl 550.21 2 MV: I-Somol (scopy/L\( smiyrtB b) 117 grams of NaCl (Z c) 87.6 grams of NaCl : O-WSOrJ\O\ 43.8 grams of NaCl \ _ l e) none of the above 58415 (OJSOWOB "' 43's 3 UQQ mm 17. What is the total number of atoms (C atoms + H atoms +,N atoms + O atoms + S atoms) present in one mole of molecules with the molecular formula CSHllNOZS ? :hmmmw s+u\+\+2.+\: 20W a) 20 atoms (0 0 [C323 b) 6.022 x 1023 atoms mm ' 21* c 5 atoms '23 t 6.022 x (0 49m MW 0 @ 1.204 x 1025 atoms m 2 e) none of the above mom MW “‘99:: 25‘ : \.2434»$(C> CflhflKVQ WWW 18. A compound contains only carbon and hydrogen. When 6 burned in an excess of oxygen, a sample of this compound gives 0.220 g of CO2 and 0.045 g of H20. What is the maximum number of moles of hydrogen atoms that could be present in this sample? Give your answer to two significant figures. 5) 5 o x 10-3 2H a H20 ' mammm H10: l8.o\31moL\-£2CD b) 2.5 x 10—3 c) 7.5 x 10-3 0.0485/Héb(\mol,HZ/O 2 nod H—ct‘qmp [8.0L8 O ‘lmoL d) 1.2 x 10-3 a e) none of the above : 5.0%‘0 _W‘ H. QW 19. In the reaction shown below, 1.50 moles of KClO3 are heated, and the reaction yield is 33.6%. How many grams of 02 are produced in this reaction? (molar mass 02 = 32.0 g/mole.) 2KClO3 —> ZKCl + 302 a) 8.06 grams of O2 l‘5omo, M03 amotoz .3 b) 72.0 grams of 02 2m“ K Md Ob c) 48.3 grams of 02 2 72.0801 ‘Vb [COO/O 24.2 grams of 02 e) none of the above . §3QC72.03023 2 20. Consider the following reaction: If you start with 12.0 g of H2 and 74.5 g of CO, how much CH3OH can be produced, assuming that the reaction goes to completion? 85.1 g co = 28.0 g/mol b) 190. g H2 = 2.02 g/mol c) 95.0 g X CH3OH = 32.0 g/mol [2.05%. ‘mo‘ 1 ,mol 301+ 32.05CH30H d) 380 9 (29251209649. 1m M )(deH H e) none of the above ‘2 015-0 swap” H ‘74.SqCD(\mo\CO \mmCHaOH X320 C“: 288% 230303 \cho WC‘WO crgofi Lkecge £212 smum. Wild—L r— 21. Avogadro's number is defined as the number of atoms in 7 a) a block of C exactly 1 cm square. b) 6.000 g of C-12. c) 14.000 g of C-14. d) exactly 12 g of naturally occurring carbon. @none of the above. MN); ll 3mm % C42 22. The classification of the following reactions in order is 4_ —— HCl(flq) + NH3(aq) ->0NH4Cl(aq) oucL‘aCMQ UQtHiO fl (0% +9: 2??gb(s) —> 82(g) + 2Hg(l) m 10am. HCl(aq) + AgNO3(aq) -9 AgCl(s) + HNO3(aq) FNQL;prEIhflT\ ’- acid—base, redox, and precipitation respectively. b) precipitation, acid—base, and redox respectively. c) redox, precipitation, and acid-base respectively. d) acid-base, precipitation, and redox respectively. e) redox, acid-base, and precipitation respectively. 23. Identify the spectator ion or ions (if any) in the redox reaction of a solution of lead(II) nitrate with zinc metal. Pb(NO3)2(aq) + Zn(s) ‘9 Zn(NO3)2(aq) + Pb(S) 2i a) Pb2+ £3294)— ggcagfzna) @ZnCaQ-y Lama +PLJC5) d) Zn and Pb metal e) no spectator ions are present 24. Which equation below best represents the balanced, net ionic equation for the reaction of a dilute solution of calcium hydroxide with a solution of hydrochloric acid? (Hint: No solids are present in the initial Ca(OH)2 solution) a) Ca2+(aq) + 2c1-(aq) —> Cac12(s) b) Ca2+(aq) + 2Cl"(aq) —> CaClz(aq) c) 20H'(aq) + 2Cl‘(aq) -9 H20(l) + OCl‘(aq) d) Ca(OH)2(aq) + 2Cl‘(aq) -9 CaC12(s) + 20H‘(aq) 6’ OH-(aq> + H+(aq) —> H20(l) , ‘ i + Q 2H + +53%: 3 133396? wager act’s/12%)) 25. 26. 27. 28. 0.0150 M Cuso4 Consider the redox reaction 8 +1 -1 o 0 +’ "' 2NaI(aq) + C12(g) -9 Iz(aq) + 2NaCl(aq) The species undergoing reduction is _ Gem 4 0— W 630mm “mm a) sodium ion. k—— b) iodide ion. <:) chlorine. C) (:J“ d) iodine . (29. + C"). A; . e) water. C}WORRQ Qfidcrm£a If 6.00 mL of 0.0250 M CuSO4 are diluted to 10.0 mL, what is the concentration of CuSO4 in the diluted solution? a) 0.00417 M Cuso4 007.80 and 6430‘; (occupy): 3:, 0.0001. c) 0.00625 M Cuso4 )‘ d) 0.0100 M Cuso4 x; 0.0150 md e) none of the above L. What are the ion concentrations in a 0.12 M solution of BaClz? B 2+ = 0.12 M d C1“ = .12 M E t 2+ -— :: EBa2+i 0 12 M and ECl ] g 060 M F33 +i2Cl a = . an ‘] = . 2. 2+ _ _ __ / \ O.2.‘-\-k @[Ba ]—0.12Mand [Cl ] —0.24M + d) [Ba2+] = 0.060 M and [Cl'] = 0.060 M 0.11 hBDLJ e) none of the above How many milliliters of 0.812 M HCl would be required to titrate 1.33 g of NaOH (molar mass = 40.00 g/mol) to the equivalence point? NaOH(aq) + HCl(aq) -9 NaCl(aq) + H20(l) 1-3391h0**(\m°\w€+0H : 0.0%3ZS‘mox khOH 40.00% b) 27.0 mL I \I +*C4 C) 1080 mL 0.0332Smok IUQOH mod HQ Y 0.03313 and d) 1640 mL .mo’ WH e) none of the above : :HcWOK M3 :itmd: o-oaszsm Ho : 0.0M?) LHq H o~<gylrno\ HG /L 29. What volume of 0.150 M NaOH is needed to react completely 9 with 3.45 g 12 (molar mass = 253.8 g/mole) according to the equation: 3I2 + _) + + ~ *‘ ~ mock 181 mL 3.45 \moV-fz emlkho _, gauge, mol ‘ a 253 '8 g 5 MOI}; '- C) 60.3 mL d) 30.2 mL V;w: 0.027\%md ©0044: 0J8}? L131” M o,‘st\MoDfi7L a '8\ml_ e) none of the above L310+‘ 30. Mg lies above Cu in the activity series of metals. Which one of the following statements is correct? (2) Mg will react with Cu2+' W “(\W m b) Cu2h will react with Mgfi. c) Mg“ will react with Cu. d) Cu will react with Mg“. e) Mg will react with Cu. Each one of the following ten questions counts 1.0 point. 31. The correct formula for strontium perbromate is z+ a a) SrBrOz Sr 6104 b) Sr(BrO)2 Svcfiwohb c) SrBrz d) Sr(BrO4 )4 none of the above 32. Which one of the following is incorrectly paired with its ionic charge? a) chloride ion (-1) b) sulfide ion (—2) c) nitride ion (-3) alxw+coqx‘h3<3W9F>E¥N d) carbide ion (-4) All of the above are correctly paired. 33. Which one of the following is incorrectly paired with its 10 34. ionic charge? a) chromate ion (—2) b) acetate ion (—1) <::)permanganate ion (—2) d) cyanide ion (—1) 2- Cd34 w- cagcoo ’ H004— e) All of the above are correctly paired. The correct name for H3PO3 is a) hydrophosphoric acid b) hypophosphoric acid c) phosphoric acid phosphorous acid e) perphosphoric acid 0&3?!» 7L afijD-57.+35CT2>;fiD x,:-C>{3-="+3 “0+ Ngmfiso 0,91? PWVQE or pththmedl 35. Which one of the following chemical formulas is not correct? 36. 37. a) CaSO4 b) NH4c1o4 @ KZASO3 d) CuC12 e) FeO 2+ 2- $<T auéLl Aégb ” C3}Zt+ 2(1- cfl< 0K FDFH: quii Q1C%T OK Feu‘ani 02— O K The correct name for C102 is a chlorine oxide b) chlorine dioxide c) chlorine(IV) oxide d) chloric oxide e) monochlorine oxide a) penta- b) tri- = c deca— = d) hepta— e) octa— = five three ten I! NM six eight ‘1 L, boom ' 2mm M when Which of one the following prefixes is incorrectly matched? 38. Which one of the following is incorrectly paired? 11 (f5 HCN = cyanic acid kgdmxufinc_dxlfifl b) HI = hydroiodic acid OK c) H2CrO4 = chromic acid 0’4 d) H28 = hydrosulfuric acid OK e) H2C03 = carbonic acid 0K 39. What is a correct formula for sodium bicarbonate? a) NazHCO3 NaHCO3 C) Na2CO3 d) NaHC02 e) none of the above 40. Then added to the name 0 mean a) more than b) the same as c) less than (:D water is included e) sulfur is substituted 0.9.90 cauLod sodxoon kgévcgn CQLWCTU 00.2503 3 Bedlam W Mecca : Sachem teammate f a salt, the word "hydrate" is used to ‘—-—\4 ...
View Full Document

Page1 / 11

[Bush] Chemistry Exam #2 - Fall 2006 - NAME 1 Chemistry...

This preview shows document pages 1 - 11. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online