W06%20Sample%20Midterm%20II

W06%20Sample%20Midterm%20II - c“ ‘1“ , \3/ Va.”...

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Unformatted text preview: c“ ‘1“ , \3/ Va.” L\I\.s "an. 2 at) :zrce» Swat» M T 17: MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following reactions is a redox reaction? A) NaOH + BC] -+ NaCl + H20 B) Pb2+ + 2C1- —+ PbClz C) AgNO3 + HQ —> HNO3 + AgCl D) (3207-2 + H20 —> 2004—2 +2H+ E) None of the above is a redox reaction. Table 20.2 Half—reaction Cr3+ (aq) + 3e“ —e Cr (s) E” (V) Fe2+(aq) + 2e- —> Fe (5) —0.440 1393+ (aq) + e' —> Fe2+ (s) +0.771 Sn4+ (aq) + 2e‘ -> Sn2+ (aq) +0.154 2) Which of the following reactions will occur spontaneously as written? A) Sn4+ (aq) + Fez"+ (aq) —> Sn2+ (aq) + 1392+ (aq) B) 3Fe(s) + 2Cr3+(aq) —> 2Cr(s) + 3Fe2+(aq) C) Sn4+ (aq) + Fe2+(aq) —> Sn2+ (aq) + Fe (5) D) C’aSn‘lt+ (aq) + 2Cr (s) -> 2Cr3+ (aq) + 38n2+ (aq) E) 3Fe2+ (aq) —> Fe (3) + 2.Fe3+ (aq) 3) A solution of an unknown Gadolinium salt was electrolyzed with a current of 1.0 amperes for 2.0 hours, depositing 3.93 grams of Gd. What is the oxidation number of Gadolinium in this salt? A) +5 B) +4 C) +3 D) +2 E) +1 4) What is the oxidation number of chromium in the dichromate ion? A) +3 B) +12 C) +7 D) +6 E) +14 5) A voltaic cell is constructed with two Zn2+—Zn electrodes, where the half—reaction is an+ + 2e- —> Zn (S) 13° = —0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 x 10‘2 M, respectively. The cell emf is V. A) —1.54 x 10‘3 B) -378 C) 0.0798 D) 0.160 E) -0.761 0 6) The reaction 2Co+3 + 2Cl‘ —> 2Co+2 + C12 has a standard voltage Eceu = + 0.46 V. For C12 + 2e" —> 2C1" , E? = + 1.36 V. What is the standard reduction potential for the reaction Co+3 + e' —> CoJr2 ? A) 1.82 V B) -0.9 C) 0.9 D) -1.82 E) —1.36 7) How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgN 03 solution using a current of 30 amps? A) 2.7 x 104 B) 3.2 x 103 C) 30 D) 3.7 x 10-5 E) 60 8) Cathodic protection of a metal pipe against corrosion usually entails A) attaching an active metal to make the pipe the anode in an electrochemical cell. B) coating the pipe with another metal whose standard reduction potential is less negative than that of the pipe. C) attaching an active metal to make the pipe the cathode in an electrochemical cell. D) attaching a dry cell to reduce any metal ions which might be formed. E) coating the pipe with a fluoropolymer to act as a source of fluoride ion (since the latter is so hard to oxidize). 9) electrons appear in the following half—reaction when it is balanced. S4062‘ —> 232032" A)6 B)2 C)4 D)1 E)3 Table 20.2 Half—reaction Ci3+ (aq) + 3e‘ —> Cr (3) E° (V) Fe2+ (aq) + Ze‘ —> Fe (3) -0.440 Fe3+ (aq) + e— —> Fe2+ (s) +0.771 Sn4+ (aq) + 2e" —-> Sn2+ (aq) +0.154 10) The standard cell potential (E°Cell) for the voltaic cell based on the reaction below is V. 2Cr (s) + 3Fe2+ (aq) -> 3Fe (s) + 2Cr3+ (aq) A) +0.30 B) +2.80 C) +3.10 D) +0.83 E) —0.16 11) The purpose of the salt bridge in an electrochemical cell is to A) maintain electrical neutrality in the half-cells via migration of ions. B) provide a source of ions to react at the anode and cathode. C) provide oxygen to facilitate oxidation at the anode. D) provide a means for electrons to travel from the anode to the cathode. E) provide a means for electrons to travel from the cathode to the anode. 12) Which transformation could take place at the anode of an electrochemical cell? A) —> 12+ B) F2 toF‘ C) Oz to H20 D) HAsOZ to As E) None of the above could take place at the anode. 13) The nitride ion is a strong Br®nsted—Lowry base. Mg3N2 reacts with water to produce A) N2 B) N20 C) NO D) N02 E) NH3 14) The principal combustion products of compounds containing carbon and hydrogen in the presence of excess 02 are A) C02 and H20 B) C02 and H202 C) C02 and H D) C(graphite) and H2 E) C02 and H2 15) An example of a form of pure carbon that contains only Sp3 hybridized carbon atoms is . A) diamond B) charcoal C) graphite D) carbon black E) carborundum 16) Silicones can be oils or rubber—like materials depending on A) the silicon-to—oxygen ratio. B) the length of the chain and degree of cross—linking. C) the percentage of carbon in the chain. D) the percentage of sulfur in the chain. E) the oxidation state of silicon in the chain. 17) Carbon dioxide is produced A) in blast furnaces when metal oxides are reduced with CO. B) by combustion of carbon—containing substances in an excess of oxygen. C) when carbonates are heated. D) by fermentation of sugar during the production of ethanol. E) by all of these processes. 18) In a group of nonmetals, which element(s) is (are) most likely to be form stable It bonds? A) the bottom element B) the top element C) the middle element D) the second element E) None of them, nonmetals do not do this. 19) How many oxygen atoms are bonded to each silicon atom in SiOz? A) 1 B) 2 C) 3 D) 4 E) none 20) Which one of the following has the lowest ionization energy? A) iodine B) bromine C) chlorine D) fluorine E) oxygen 21) Boron can violate the octet rule in its compounds in that A) it can have an expanded octet. B) it can exist in a molecule with an odd number of electrons. C) its compounds are all ionic. D) it can have fewer than eight valence electrons. E) boron cannot violate the octet rule. 22) The electron—pair geometry and molecular geometry of Xer are and respectively. A) trigonal bipyramidal; bent B) trigonal bipyramidal; linear C) trigonal bipyramidal; bent D) octahedral; linear E) octahedral; bent 23) The heavier noble gases are more reactive than the lighter ones because A) the lighter noble gases exist as diatomic molecules. B) the lighter noble gases have complete octets. C) the heavier noble gases are more abundant. D) the heavier noble gases have low ionization energies relative to the lighter ones. E) the heavier noble gases have greater electron affinities. 24) Which property of metals cannot be explained with the electron—sea model? A) shine B) high thermal conductivity C) high electrical conductivity D) malleability and ductility E) trends in melting points 25) What is produced when a carbonate is calcined? A) the free metal and sodium carbonate B) the free metal and sulfur dioxide C) the metal oxide and carbon dioxide D) water and the metal hydride E) the free metal and carbon dioxide 26) An advantage to leaching gold with aqueous solutions of cyanide ion is that A) the process requires only one step. B) the gold recovered in this way has higher purity than gold recovered in other ways. C) the method can be used to locate underground gold deposits. D) gold can be recovered from very low-grade ores by this method. E) the process is environmentally safe. 27) If the electronic structure of a solid substance consists of a valence band that is partially filled with electrons and there is a small energy gap to the next set of orbitals, then this substance will be a(n) A) alloy B) insulator C) conductor D) semiconductor E) nonmetal 28) Alloys generally differ from compounds in that A) the former always contain some carbon. B) the former always contain some iron. C) the former always have semiconductor properties. D) the atomic ratios of the constituent elements in the former are not fixed and may vary over a wide range. E) the former never contain a transition element. 29) Gold and the platinum group metals are found in nature in metallic form because A) they are solids at room temperature. B) they are highly reactive. C) they are soluble in water. D) they are relatively inert. E) they are relatively abundant. Chemistry 123 Some Potentially Useful Information Gas Constant, R = 8.314 J/mol ’K 1 Faraday, F = 96,500 Coulombs Gibbs Free Energy, AG0 = AH0 - TAS0 Speed of Light, c = 2.998 x 108 m/sec Nemst Equation: Bee" = E056“ — 0.0592/n (logQ) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) E ID: chem9b 20.1—6 Page Ref: Sec. 20.1 2) D ID: chem9b 201—47 Page Ref: Sec. 20.5 3) C ID: chem9b 20.2-10+ Page Ref: Sec. 20.9 4) D ID: chem9b 201—10 Page Ref: Sec. 20.1 5) C ID. d1em9b 202-?» Page Ref: Sec. 20.6 6) A ID: chem9b 20.1-65+ Page Ref: Sec. 20.9 7) C ID: chem9b 20.1—64 Page Ref: Sec. 20.9 8) C ID: cheme 20.1—57 Page Ref: Sec. 20.8 9) B ID: chem9b 201-14 Page Ref: Sec. 20.2 10) A ID: chem9b 201—43 Page Ref: Sec. 20.4 1 1) A ID: chem9b 20.1—27 Page Ref: Sec. 20.3 12) E ID: chem9b 20.1-26 Page Ref: Sec. 20.3 13) E ID: chem9b 221—79 Page Ref: Sec. 2.7 14) A ID: chem9b 221—108 Page Ref: Sec. 22.9 15) A ID. chem9b 221—120 Page Ref: Sec 2.9 16) B ID. chem9b 221-150 Page Ref: Sec. 22.10 17) E ID: chem9b 221—124 Page Ref: Sec. 22.9 18) B II) chem9b 22.1—1 Page Ref: Sec. 22.1 19) 3 D ID. chem9b 221—5 Page Ref: Sec. 22.1 20) t A ID: chem9b 22.1~8 Page Ref: Sec. 221 21) D ID: chem9b 221—162 Page Ref: Sec. 22.11 22) B ID: chem9b 22.1—34+ Page Ref: Sec. 2.3 23) D ID: chem9b 221—41 Page Ref: Sec. 22.3 24) E ID: chem9b 231—71 Page Ref: Sec. 23.5 25) C ID: chem9b 231—25 Page Ref: Sec. 23.2 26) D ID: Chem9b 231—53 Page Ref: Sec. 23.3 27)‘C. ID. chem9b 231—74 Page Ref: Sec. 23.5 28) D ID: chem9b 23.1—83 Page Ref: Sec. 23.6 29) D ID: chem9b 231—15 Page Ref: Sec. 23.1 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) E ID: chem9b 20.1-6 Page Ref: Sec. 20.1 2) D ID: chem9b 20.1—47 Page Ref: Sec. 205 3) C ID: chem9b 20.2- 10+ Page Ref: Sec. 20.9 4) D ID: chem9b 20.1-10 Page Ref: Sec. 20.1 5) C III chem9b 202—31 Page Ref: Sec. 20.6 6) A ID: Chem9b 20.1—65+ Page Ref: Sec. 20.9 7) C ID: chem9b 20.1—64 Page Ref: Sec. 20.9 8) C ID: chem9b 20.1—57 Page Ref: Sec. 20.8 9) B ID chem9b 20.1—14 Page Ref: Sec. 20.2 10) A ID: chem9b 20.1—43 Page Ref: Sec. 20.4 11) A ID: chem9b 201—27 Page Ref: Sec. 20.3 12) E ID: chem9b 20.1-26 Page Ref: Sec. 20.3 13) E ID: Chem9b 221—79 Page Ref: Sec. 2.7 14) A ID: (111811191) 221—108 Page Ref: Sec. 22.9 15) A ID: chem9b 221—120 Page Ref: Sec. 2.9 16) B ID: chem9b 221—150 Page Ref: Sec. 22.10 17) E ID: chem9b 221—124 Page Ref: Sec. 229 18) B ID: chem9b 22.1—1 Page Ref: Sec. 2.1 19) It D ID: chem9b 22.1-5 Page Ref: Sec. 22.1 20) ‘ A In chem9b 22.14; Page Ref: Sec. 2.1 21) D ID: chem9b 221—162 Page Ref: Sec. 2211 22) B ID: chem9b 22.1—34+ Page Ref: Sec. 223 23) D ID: chem9b 221-41 Page Ref: Sec. 223 24) E ID: chem9b 23.1—71 Page Ref: Sec. 23.5 25) C ID: chem9b 23.1—25 Page Ref: Sec. 232 26) D ID: chem9b 23.1—53 Page Ref: Sec. 23.3 27) x‘ C. ID: Chem9b 23.1—74 Page Ref: Sec. 23.5 28) D ID chem9b 23.1—83 Page Ref: Sec. 23.6 29) D ID: chem9b 23.1-15 Page Ref: Sec. 23.1 ...
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This note was uploaded on 04/10/2008 for the course CHEM 123 taught by Professor Larosa during the Spring '06 term at Ohio State.

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W06%20Sample%20Midterm%20II - c“ ‘1“ , \3/ Va.”...

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