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Electrochemistry Multiple Choice
January 1999
37. Consider the following redox reaction:2MnO4
- + 3ClO3- + H2O 3ClO4
- + 2MnO2 + 2OH-
The reducing agent is
A. H2OB. ClO3
-
C. MnO2
D. MnO4-
38. Consider the following reaction that occurs in a breathalyzer:2Cr2O7
2-(aq) + 16H+
(aq) + 3C2H5OH(g) 4Cr3+(aq) + 11H2O(l) + 3CH3COOH(aq)
Which atom undergoes an increase in oxidation number?
A. carbonB. oxygenC. hydrogenD. chromium
39. Which of the following is the strongest reducing agent?
A. AlB. CuC. ZnD. Mg
40. Which of the following reactions is spontaneous at standard conditions?
A. Pb + Cu2+ Cu + Pb 2+
B. H2 + Mg2+ Mg + 2H+
C. Br2 + 2Cl- Cl2 + 2Br-
D. 2Ag + Cu2+ Cu + 2Ag+
41. Consider the following redox reaction:3ClO2
- 2ClO3- + Cl- (basic)
The reduction half-reaction that occurs is
A. ClO2- + 2H2O + 4e- Cl- + 4OH-
B. ClO2- + 2H2O Cl- + 4OH- + 4e-
C. ClO2- + 2OH- + 2e- ClO3
- + H2OD. ClO2
- + 2OH- ClO3- + H2O + 2e-
42. Vanadium metal, V, reacts spontaneously with Cd2, but not with Ti2. Based on these results, the order of oxidizing agents, from strongest to weakest, is
A. Cd2+, V2+, Ti2+
B. V2+, Ti2+ , Cd2+
C. Ti2+, Cd2+, V2+
D. Ti2+, V2+, Cd2+
43. Consider the following electrochemical cell:
In this operating electrochemical cell,
A. electrons flow toward the Cu and the Cu2ions migrate toward the Zn.B. electrons flow toward the Cu and the Zn2ions migrate toward the Cu.C. electrons flow toward the Zn and the Cu2ions migrate toward the Zn.D. electrons flow toward the Zn and the Zn2ions migrate toward the Cu.
44. Which of the following affects the potentials of electrochemical cells?
A. I and II only.B. II and III only.C. I and III only.D. I, II and III.
45. In the rusting of iron, the reduction reaction that occurs is
A. Fe Fe2+ + 2e-
B. Fe2+ + 2e- FeC. 2H2O O2 + 4H+ + 4e-
D. O2 + 2H2O + 4e- 4OH-
46. During a cathodic protection, the sacrificial anode
A. accepts electrons from the protected metal.B. reacts spontaneously with the protected metal.C. oxidizes more readily than the protected metal.D. causes the protected metal to become an anode.
47. During the electrolysis of an aqueous solution of KI, what substance is formed at the cathode?
A. iodineB. oxygenC. hydrogenD. potassium
48. When electroplating an iron medallion with nickel,
A. the medallion is an anode.B. the cathode is pure nickel.C. the solution contains Ni2.D. the anode reaction is Ni22eNi
April 1999
37. Which of the following represents the formation of a stronger acid as a result of oxidation?
A. H2SO3 H2SB. HClO4 HClC. H2SO3 H2SO4
D. HCO3- H2CO3
38. Chlorine has an oxidation number of 5 inA. NaClOB. NaClO2
C. NaClO3
D. NaClO4
39. Consider the following:NO2 N2O3
The nitrogen atom in each NO2
A. loses one electron.B. gains one electron.
C. loses two electrons.D. gains two electrons.
40. Which of the following is the strongest oxidizing agent?
A. BrO3- C. S2O8
2-
B. ClO4- D. Cr2O7
2-
41. Consider the following half-reaction:1 AsH3 + __ H2O __ H3AsO3 + ? H+ + __e-
When this half-reaction equation is balanced, the coefficient for His
A. 2B. 3C. 6D. 9
42. When a strip of zinc is placed in a 1.0M copper (II) chloride solution,
A. no change occurs.B. the [Clincreases.C. the [Cu2increases.D. the [Zn2increases.43. Consider the following electrochemical cell:
What changes occur when the cell is in operation?
44. A redox titration is performed in order to determine the [H2O2].Which of the following would not be a suitable reagent to use?
A. acidified IO3-
B. acidified SO42-
C. acidified MnO4-
D. acidified Cr2O72-
45. Ethanol, C2H5OH, is oxidized by an acidified dichromate solution according to the following equation:2Cr2O72- + 16H+ + 3C2H5OH 4Cr3+ + 11H2O + 3CH3COOH
The Efor the reaction above is 2.98V. The Efor the oxidation of ethanol is
A. 0.52VB. 1.23VC. 1.75VD. 2.98V
46. Which of the following must be present to produce rust by the corrosion of iron?
A. I onlyB. II onlyC. I and II onlyD. I, II and III
47. Why can an object not be plated with magnesium using 1.0M MgI2?
A. Water is a stronger reducing agent than I
B. Water is a stronger oxidizing agent than I
C. Water is a stronger reducing agent than Mg2
D. Water is a stronger oxidizing agent than Mg2
48. In the electrolysis of 1.0M Na2SO4, what is formed at the cathode?
A. O2
B. H2
C. H2SO3
D. S2O82-
June 1999
37. Which of the following is capable of acting both as an oxidizing agent and a reducing agent?
A. H+
B. Na+
C. Sn2+
D. MnO4-
38. Consider the following redox reaction:C2H12O6 + 6O2 6CO2 + 6H2O
The substance undergoing reduction is
A. O2
B. CO2
C. H2OD. C6H12O6
39. The oxidation number of P in H4P2O7 is
A. -10B. -5C. +5D. +10
40. A solution containing an unknown cation reacts spontaneously with both zinc and copper. The unknown cation is
A. 1.0M H+
B. 1.0M Ag+
C. 1.0M Sr2+
D. 1.0M Mn2+
41. Which of the following half-reactions is balanced?
A. CIO- + H2O +e- Cl2 + 2OH-
B. 2CIO- + H2O +2e- Cl2 + 3OH-
C. 2CIO- + 2H2O +2e- Cl2 + 4OH-
D. 2CIO- + 2H2O Cl2 + 4OH- + 2e-
42. Which of the following is a spontaneous redox reaction?
A. Ag+ + I- AgIB. Ag+ + Fe2+ Ag + Fe3+
C. 3Ag+ + Au 3Ag + Au3+
D. 2Ag+ + Ni2+ 2Ag + Ni
43. Salting of roads during the winter increases the corrosion of cars.
This is because the salt
A. reacts with the iron.B. provides an electrolyte.C. acts as a reducing agent.D. acts as an oxidizing agent.
44. Which of the following will not react spontaneously with 1.0M HCl?A. tinB. lithiumC. mercuryD. aluminum
45. Consider the following electrochemical cell:
The half-reaction that occurs at the anode is
A. Ni Ni2+ + 2e-
B. Ni2+ + 2e- NiC. Cu Cu2+ + 2e-
D. Cu2+ + 2e- Cu
46. Which of the following can be produced by electrolysis from a 1.0M aqueous solutioncontaining its ion?
A. nickelB. sodiumC. aluminumD. magnesium
47. In the electrolysis of molten ZnCl2 using carbon electrodes, the reaction that occursat the anode is
A. Zn Zn2+ + 2e-
B. Zn 2+ + 2e- ZnC. 2Cl- Cl2 + 2e-
D. Cl2 + 2e- 2Cl-
48. In order for an electrolytic cell to operate, it must have
A. a voltmeter.B. a salt bridge.C. a power supply.D. an aqueous solution.
August 1999
38. The following reaction represents the process used to produce iron from iron (III) oxide:Fe2O3 + 3CO 2Fe + 3CO2
What is the reducing agent in this process?
A. FeB. COC. CO2
D. Fe2O3
39. Consider the following reaction:2HNO2 + 2I- + 2H+ 2NO + I2 + 2H2O
The oxidation number for each nitrogen atom
A. increases by 1B. increases by 2C. decreases by 1D. decreases by 2
40. Which of the following reactions is spontaneous?
A. 2I- + Ag Ag+ + I2
B. Co2+ + Cu Co + Cu2+
C. Cu2+ + Pb Pb2+ + CuD. Ni2+ + 2Ag 2Ag+ + Ni
41. Consider the following redox reaction for a lead-acid storage cell:Pb + PbO2 + 4H+ + 2SO4
2- 2PbSO4 + 2H2OThe balanced, reduction half-reaction is
A. Pb + SO42- PbSO4 + 2e-
B. Pb + 2H+ + SO42- PbSO4 + H2O + 2e-
C. PbO2 + 4H+ + SO42- + 2e- PbSO4 + 2H2OD. PbO2 + SO4
2- + 4H2O + 2e- PbSO4 + 4OH-
Use the following diagram to answer questions 42 and 43.
42. Which of the following statements apply to this electrochemical cell?
A. I and II onlyB. I and III onlyC. II and III onlyD. I, II and III
43. At equilibrium, the voltage of the cell above is
A. 1.10 VB. 0.00 VC. 0.42 VD. 1.10 V
44. Consider the following reaction:Cd2+
(aq) + Zn (s) Cd(s) + Zn 2+ (aq)
The potential for the reaction is 0.36V. What is the reduction potential for the cadmium ion?
A. 1.12 VB. 0.40 VC. 0.40 VD. 1.12 V
45. Which of the following involves a non-spontaneous redox reaction?
A. fuel cellB. electroplatingC. redox titrationD. carbon dry cell
46. Consider the following redox reaction:2MnO4
- + 16H+ + 5Sn2+ 2Mn2+ + 8H2O + 5Sn4+
In a redox titration, 0.060 mol of KMnO4 reacts completely with a solution of Sn(NO3)2 .How many moles of Sn(NO3)2 were present in the solution?
A. 0.024 molB. 0.060 molC. 0.15 molD. 0.30 mol
47. What substances are formed at the anode and cathode during electrolysis of moltensodium chloride, NaCl (l)?
48. What is the minimum voltage required to form nickel from an aqueous solution of NiI2 using inert electrodes?
A. 0.26V C. 0.54VB. 0.28V D. 0.80V
January 2000
38. Which of the following represents a redox reaction?
A. CaCO3 CaO + CO2
B. SiCl4 + 2Mg Si + 2MgCl2
C. 2NaOH + H2SO4 2H2O + Na2SO4
D. AgBr + 2S2O32- Ag(S2O3)2
3- + Br-
39. Consider the following reaction:TiCl4 + O2 TiO2 + 2Cl2
Each oxygen atom is
A. reduced and loses 2e-
B. reduced and gains 2e-
C. oxidized and loses 2e-
D. oxidized and gains 2e-
40. When NO2 acts as a reducing agent, a possible product is
A. NOB. N2OC. N2O4
D. N2O5
41. Which of the following 1.0M solutions will react spontaneously with lead?
A. KClB. CuCl2
C. ZnCl2
D. MgCl2
42. Consider the following redox reaction:I2 + 2S2O3
2- S4O62- + 2I-
In a titration, 40.00mL of Na2S2O3 is needed to react completely with 4.0 X 10-3 mol I2.What is the concentration of Na2S2O3?
A. 0.10MB. 0.16MC. 0.20MD. 0.32M
43. In an operating electrochemical cell the function of a salt bridge is to
A. allow hydrolysis to occur.B. allow a non-spontaneous reaction to occur.C. permit the migration of ions within the cell.D. transfer electrons from the cathode to the anode.
Use the following diagram to answer questions 44 and 45.
44. As the cell operates, electrons flow toward
A. the Pb electrode, where Pb is oxidized.B. the Cd electrode, where Cd is oxidized.C. the Pb electrode, where Pb2+ is reduced.D. the Cd electrode, where Cd2+ is reduced.
45. The E° value for the reduction of Cd2+ is
A. –0.40VB. –0.27VC. +0.14VD. +0.40V
46. The following reaction occurs in an electrochemical cell:3Cu2+ + 2Cr 2Cr3+ + 3Cu
The E° for the cell is
A. 0.40V C. 1.08VB. 0.75V D. 2.50V
47. During the corrosion of magnesium, the anode reaction is
A. Mg Mg2+ + 2e-
B. Mg2+ + 2e- MgC. 4OH- O2 + 2H2O + 4e-
D. O2 + 2H2O + 4e- 4OH-
48. A molten binary salt, ZnCl2, undergoes electrolysis. The cathode reaction is
A. Zn Zn2+ + 2e-
B. 2Cl- Cl2 + 2e-
C. Cl2 + 2e- 2Cl-
D. Zn2+ + 2e- Zn
April 2000
38. Manganese has an oxidation number of +4 in
A. MnOB. MnO2
C. Mn2O3
D. Mn2O7
39. In which reaction is nitrogen reduced?
A. 2NO + O2 2NO2
B. 4NH3 + 5O2 4NO + 6H2OC. Cu2+ + 2NO2 + 2H2O Cu + 4H+ + 2NO3
-
D. 4Zn + 10H+ + NO3- 4Zn2+ + NH4
+ + 3H2O
40. An oxidizing agent will cause which of the following changes?
A. PtO2 PtOB. PtO3 PtO2
C. Pt(OH)2 Pt
D. Pt(OH)22+
PtO3
41. Consider the overall reaction of the rechargeable nickel-cadmium battery:NiO2(s) + Cd(s) + 2H2O(l) Ni(OH)2(s) + Cd(OH)2 (s)
Which of the following occurs at the anode as the reaction proceeds?
A. Cd loses 2e- and forms Cd(OH)2 (s)
B. Cd gains 2e- and forms Cd(OH)2 (s)
C. NiO2 loses 2e- and forms Ni(OH)2 (s)
D. NiO2 gains 2e- and forms Ni(OH)2 (s)
42. Which of the following will oxidize Fe2+?A. I2 (s)
B. Ni (s)
C. Zn(s)
D. Br2(l)
43. Consider the following half-reaction in a basic solution:Ag2O3 AgO (basic)
The balanced half-reaction is
A. Ag2O3 + 4H+ + 4e- AgO + 2H2OB. Ag2O3 + 2H+ + 2e- 2AgO + H2OC. Ag2O3 + H2O + 2e- 2AgO + 2OH-
D. Ag2O3 + 2H2O + 4e- AgO + 4OH-
44. The concentration of Fe2+ (aq) can be determined by a redox titration using
A. KBrB. SnCl2
C. KMnO4 (basic)D. KBrO3 (acidic)
45. Consider the following electrochemical cell:
Which of the following occurs as the cell operates?
A. Zinc electrode is reduced and increases in mass.B. Zinc electrode is reduced and decreases in mass.C. Zinc electrode is oxidized and increases in mass.D. Zinc electrode is oxidized and decreases in mass.
46. Which of the following reactants would produce an E° of +0.63V?
A. Ag+ + I2
B. Pb2+ + ZnC. Mg2+ + CaD. Zn2+ + Mn
47. The process of applying an electric current through a cell to produce a chemical change is called
A. corrosion.B. ionization.C. hydrolysis.D. electrolysis
48. Consider the following electrolytic cell:
The cathode reaction is
A. 2I- I2 + 2e-
B. Mg2+ + 2e- MgC. H2O ½O2 + 2H+ + 2e-
D. 2H2O + 2e- H2 + 2OH-
June 2000
38. A substance that is reduced during a redox reaction
A. loses mass.B. is the anode.C. is the reducing agent.D. is the oxidizing agent.
39. The oxidation number of As in H4As2O7 is
A. +4B. +5C. +9D. +10
40. In a reaction, the oxidation number of Cr decreases by 3. This indicates that Cr is
A. reduced.B. oxidized.
C. neutralized.D. a reducing agent.
41. Consider the following redox reaction:C2H5OH + 2Cr2O7 2- + 16H+ 2CO2 + 4Cr3+ + 11H2O
Each carbon atom loses
A. 2 electronsB. 4 electronsC. 6 electronsD. 12 electrons
42. In which of the following 1.0M solutions will both ions react spontaneously with tin?
A. Ag+ and Cu2+
B. Ni2+ and Cu2+
C. Zn2+ and Ni2+
D. Mg2+ and Zn2+
43. Consider the following half-reaction:Bi2O4 BiO+ (acidic)
The balanced equation for this half-reaction is
A. Bi2O4 + 6H+ + 5e- BiO+ + 3H2OB. Bi2O4 + 8H+ + 6e- 2BiO+ + 4H2OC. Bi2O4 + 4H+ + 2e- 2BiO+ + 2H2OD. Bi2O4 + 4H+ + 3e- 2BiO+ + 2H2O
44. To determine the concentration of Fe2+(aq) by a redox titration, we could use an acidified standard solution of
A. Sn2+
B. Pb2+
C. HClD. H2O2
45. Consider the following redox reactions:
2Ag+ + Cd 2Ag + Cd2+ E° = 1.20V3Cd2+ + 2Nb 2Nb3+ + 3Cd E° =0.70V
What is the E° for Nb3+ + 3e- Nb?
A. –1.90V C. –0.50VB. –1.10V D. –0.40V
46. Consider the overall reaction for the rechargeable nickel-cadmium battery:Cd + NiO2 + 2H2O Cd(OH)2 + Ni(OH)2
Which of the following occurs at the cathode as the reaction proceeds?
A. Cd loses 2e- and Cd(OH)2 formsB. Cd gains 2e- and Cd(OH)2 formsC. NiO2 loses 2e- and Ni(OH)2 formsD. NiO2 gains 2e- and Ni(OH)2 forms
47. Consider the following diagram of a piece of iron, cathodically protected by magnesium:
What is happening during this process?
A. Iron acts as the anode and water is oxidized.B. Iron acts as the cathode and oxygen is reduced.C. Magnesium acts as the anode and iron is oxidized.D. Magnesium acts as the cathode and iron is reduced.
48. Consider the following operating cell:
Which of the following describes the cell above?
August 2000
37. A chemical process involving the loss of electrons is a definition of
A. oxidation.B. reduction.C. galvanization.D. cathodic protection.
38. Which of the following is not a redox reaction?
A. 2Mg + O2 2MgOB. SO3 + H2SO4 H2S2O7
C. CuS + 2O2 + C Cu + SO2 + CO2
D. 4Ag + 2H2S + O2 2Ag2S + 2H2O
39. A reducing agent will cause which of the following changes?
A. ClO3- ClO2
B. NO2- N2O4
C. H3PO3 H3PO4
D. HS2O4- H2SO3
40. The oxidation number of zinc in a reaction increases by 2. This indicates that
A. zinc is reduced and loses 2 electrons.B. zinc is reduced and gains 2 electrons.C. zinc is oxidized and loses 2 electrons.D. zinc is oxidized and gains 2 electrons.
41. Which metal will react spontaneously with water?
A. CaB. NiC. PbD. Hg
42. Consider the following redox reaction which occurs in a lead-acid storage cell:PbO2(s) + Pb (s) + 2H2SO4 (aq) 2PbSO4(s) + 2H2O (s)
The balanced reduction half-reaction is
A. Pb Pb2+ + 2e-
B. Pb + SO42- PbSO4 + 2e-
C. 2H2SO4 + 2Pb + 2e- 2PbSO4 + 2H2OD. PbO2 + 4H+ + SO4
2- + 2e- PbSO4 + 2H2O
43. Consider the following redox reactions:HClO + I- HIO + Cl- E° = +0.49V
HClO + Br- HBrO + Cl- E° = +0.15VThe relative strength of the oxidizing agents from strongest to weakest is
A. HIO > HBrO > HClOB. HClO > HIO > HBrOC. HBrO >HIO > HClOD. HClO > HBrO > HIO
44. Consider the following diagram of a fuel cell in which H2 and O2 combine to produce H2O under basic conditions:
The reaction at the anode is
A. 2H+ + 2e- H2
B. ½ O2 + 2H+ + 2e- H2OC. 4OH- O2 + 2H2O + 4e-
D. H2 + 2OH- 2H2O + 2e-
45. As the cell operates, observations include
46. What is the cell potential, E°, for this cell?
A. 0.08 VB. 0.26 VC. 0.60 VD. 0.78 V
47. Consider the following electrolytic cell:
In the cell above,
A. I- migrates to the anode and gains electrons.B. I- migrates to the cathode and loses electrons.C. Na+ migrates to the anode and loses electrons.D. Na+ migrates to the cathode and gains electrons.
48. Which of the following are necessary for electroplating to occur using an electrolytic cell?
A. I and II only.B. I and III only.C. II and III only.D. I, II, and III.
January 2001
38. Which of the following represents a redox reaction?
A. C + O2 CO2
B. H2O + SO2 H2SO3
C. H3O+ +OH- 2H2OD. NaCl + AgNO3 AgCl + NaNO3
39. The oxidation number of each chromium atom in Cr2O72- is
A. +5
B. +6C. +7D. +12
40. List the ions Co2+, Cu2+ and Zn2+ in order from strongest to weakest oxidizing agents.
A. Zn2+ > Co2+ > Cu2+
B. Co2+ > Cu2+ > Zn2+
C. Cu2+ > Zn2+ > Co2+
D. Cu2+ > Co2+ > Zn2+
41. A piece of Cu reacts spontaneously with 1.0M Pd2+ because
A. Cu is a weaker reducing agent than Pd and E° > 0.B. Cu is a weaker reducing agent than Pd and E° < 0.C. Cu is a stronger reducing agent than Pd and E° > 0.D. Cu is a stronger reducing agent than Pd and E° < 0.
42. Which two species will not react spontaneously at standard conditions?
A. Co with Cl2
B. Cu with Ag+
C. Ag with Zn2+
D. Mg with Cr3+
43. When a piece of Ag is placed in 1.0M NiCl2,
A. the [Cl-] increases.B. the [Ag+] decreases.C. the [Ni2+] decreases.D. no change occurs.
44. Which of the following represents the relationship between [NO3-] and the mass of the Cu electrode in the
complete cell as it operates?
45. The E° for the above cell is
A. –1.10 VoltsB. –0.42 VoltsC. +0.42 VoltsD. +1.10 Volts
46. Which of the following is correct for an electrolytic cell?
47. Which of the following will inhibit the corrosion of iron?
A. high [O2(aq)]B. wet conditionsC. coating with zincD. increasing the temperature
48. The products of the electrolysis of molten MgCl2 using inert electrodes are
A. hydrogen and oxygen.B. hydrogen and chlorine.C. magnesium and oxygen.D. magnesium and chlorine.
April 2001
38. Consider the following reaction:Zn (s) + 2H+ (aq) Zn2+ (aq) + H2
(g)
The species being oxidized is
A. H2
B. H+
C. ZnD. Zn2+
39. When SO42- reacts to form S2O6
2-, the sulphur atoms
A. lose electrons and are reduced.B. gain electrons and are reduced.C. lose electrons and are oxidized.D. gain electrons and are oxidized.
40. Which of the following is a list of metals in order from strongest to weakest reducing agents?
A. Au > Ni > RbB. Ni > Au > RbC. Ni > Rb > AuD. Rb > Ni > Au
41. Consider the following spontaneous reaction:Mg (s) + 2HCl (aq) MgCl2 (aq) + H2(g)
Which of the following statement is correct?
A. Mg is a weaker reducing agent than H2
B. Mg is a weaker reducing agent than H+
C. Mg is a stronger reducing agent than H2
D. Mg is a stronger reducing agent than H+
42. Which of the following will not react spontaneously with H2O at standard conditions?
A. F2
B. CaC. NaD. Sn
43. When a piece of Cu is placed in 1.0M AgNO3,
A. the [Ag+] increases.B. the [Cu2+] increases.C. the [NO3
-] decreases.D. no change occurs.
44. Which of the following diagrams represents the relationship between [Ni2+] and the mass of the Cu electrode as the cell above is in operation?
45. The E° for the above cell is
A. –0.04 voltsB. –0.60 voltsC. +0.04 voltsD. +0.60 volts
46. Which of the following describes an electrochemical cell?
47. Which of the following aqueous solutions should not be used as an electrolyte in an electrolytic cell?
A. 1.0M KOHB. 1.0M H2SO4
C. 1.0M CuSO4
D. 1.0M C6H12O6
48. When 1.0M Na2SO4 is electrolyzed, the solution near the anode becomes
A. basic and bubbles form.B. acidic and bubbles form.C. basic and no bubbles form.D. acidic and no bubbles form.
June 2001
38. Which of the following represents a redox reaction?
A. H2 + I2 2HIB. HCl + NH3 NH4ClC. H2O + CO2 H2CO3
D. 2NaI + Pb(NO3)2 PbI2 + 2NaNO3
39. In an experiment, Ag+ reacts spontaneously with Ru but not with Pd. The relative strength of the metals from strongest to weakest reducing agent is
A. Ag > Ru > PdB. Pd > Ag > RuC. Ru > Ag > PdD. Ru > Pd > Ag
40. A piece of Ag does not react spontaneously with 1.0M Ti2+ because
A. Ag+ is a weaker reducing agent than Ti2+
B. Ag+ is a weaker oxidizing agent than Ti2+
C. Ag+ is a stronger reducing agent than Ti2+
D. Ag+ is a stronger oxidizing agent than Ti2+
41. Which of the following will react spontaneously with Ag2S at standard conditions?
A. AlB. AuC. CoD. Pb
42. When a piece of Cu is placed in 1.0M HNO3,
A. the [H+] increases.B. the [Cu2+] decreases.C. the [NO3
-] decreases.D. no change occurs.
43. When MnO2 changes to Mn2O3 in an alkaline battery, manganese atoms
A. lose electrons and are reduced.B. gain electrons and are reduced.C. lose electrons and are oxidized.D. gain electrons and are oxidized.
44. Which of the following diagrams represents the relationship between the mass of the Cu electrode and the mass of the Ag electrode as the cell is in operation?
45. The E° for the above cell is
A. -1.14 VoltsB. -0.46 VoltsC. +0.46 VoltsD. +1.14 Volts
46. The value of E° for a cell can be used to determine
A. rate.B. spontaneity.C. temperature.D. activation energy.
47. How is the formation of rust on an iron can inhibited by a tin coating?
A. The tin is a sacrificial anode.B. The tin cathodically protects the iron.C. The tin is a weaker reducing agent than iron.D. The tin keeps the oxygen away from the iron.
48. The electrolysis of 1.0M CuF2 using inert electrodes will produce
A. copper and oxygen.B. copper and fluorine.C. hydrogen and oxygen.D. hydrogen and fluorine.
August 2001
38. Consider the following spontaneous reaction:2Al (s) + 3Cu2+ (aq) 2Al3+
(aq) + 3Cu(s)
In this reaction, the oxidizing agent is
A. AlB. CuC. Al3+
D. Cu2+
39. Bromine has an oxidation number of +3 in
A. KBrOB. KBrO2
C. KBrO3
D. KBrO4
40. In an experiment, Te reacts spontaneously with Ag+ but not with Ti2+. The relative strength of oxidizing agents from strongest to weakest is
A. Ag+ > Te4+ > Ti2+
B. Ag+ > Ti2+ > Te4+
C. Te4+ > Ti2+ > Ag+
D. Ti2+ > Te4+ > Ag+
41. A piece of Au does not react spontaneously with 1.0M HCl. Which of the following statements is true?
A. Au is a weaker reducing agent than H2
B. Au is a stronger reducing agent than H2
C. Au is a weaker oxidizing agent than H+
D. Au is a stronger oxidizing agent than H+
42. Which two species will react spontaneously with each other at standard conditions?
A. Cl2 and Br-
B. Zn and Al3+
C. Au and Sn2+
D. I2 and SO42-
43. What occurs when a piece of Zn is placed in 1.0M Cu(NO3)2?
A. [Cu2+] decreasesB. [Zn2+] decreasesC. [NO3
-] increasesD. no change occurs
44. Which of the following diagrams represents the relationship between [Zn2+] and [Ni2+] as the cell is in operation?
45. The E° for the cell in the diagram is
A. -1.02 Volts C. +0.50 VoltsB. -0.50 Volts D. +1.02 Volts
46. Which of the following does not affect the cell potential?
A. [Ni2+] C. temperatureB. [Zn2+] D. surface area of the electrodes
47. What type of ions move toward each electrode in an electrolytic cell?
48. The electrolysis of 1.0M NaI using inert electrodes will produce
A. sodium and iodine. C. hydrogen and iodine.B. sodium and oxygen. D. hydrogen and oxygen.
January 1999 April 1999 June 1999 August 1999Question Answer Question Answer Question Answer Question Answer37 B 37 C 37 C 37 D38 A 38 C 38 A 38 B39 D 39 B 39 C 39 C40 A 40 C 40 B 40 C41 A 41 C 41 C 41 C42 A 42 D 42 B 42 D43 B 43 A 43 B 43 B44 D 44 B 44 C 44 B45 D 45 C 45 A 45 B46 C 46 C 46 A 46 C47 C 47 D 47 C 47 D48 C 48 B 48 C 48 D
January 2000 April 2000 June 2000 August 2000Question Answer Question Answer Question Answer Question Answer38 B 38 B 38 D 37 A39 B 39 D 39 B 38 B40 D 40 D 40 A 39 A41 B 41 A 41 C 40 C42 C 42 D 42 A 41 A43 C 43 C 43 C 42 D44 C 44 D 44 D 43 D45 A 45 D 45 B 44 D46 C 46 B 46 D 45 B47 A 47 D 47 B 46 C48 D 48 D 48 A 47 D
48 D
January 2001 April 2001 June 2001 August 2001Question Answer Question Answer Question Answer Question Answer38 A 38 C 38 A 38 D39 B 39 B 39 C 39 B40 D 40 D 40 D 40 A41 C 41 C 41 A 41 A42 C 42 D 42 C 42 A43 D 43 B 43 B 43 A44 B 44 A 44 A 44 C45 D 45 D 45 C 45 C46 D 46 A 46 B 46 D47 C 47 D 47 D 47 A48 D 48 B 48 A 48 C
