Electrochemistry Multiple Choice
January 1999
37. Consider the following redox reaction:
2MnO4- + 3ClO3- + H2O  3ClO4- + 2MnO2 + 2OHThe reducing agent is
A. H2O
B. ClO3C. MnO2
D. MnO438. Consider the following reaction that occurs in a breathalyzer:
2Cr2O72-(aq) + 16H+(aq) + 3C2H5OH(g)  4Cr3+(aq) + 11H2O(l) + 3CH3COOH(aq)
Which atom undergoes an increase in oxidation number?
A. carbon
B. oxygen
C. hydrogen
D. chromium
39. Which of the following is the strongest reducing agent?
A. Al
B. Cu
C. Zn
D. 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 + 2BrD. 2Ag + Cu2+  Cu + 2Ag+
41. Consider the following redox reaction:
3ClO2-  2ClO3- + ClThe reduction half-reaction that occurs is
A. ClO2- + 2H2O + 4e-  Cl- + 4OHB. ClO2- + 2H2O  Cl- + 4OH- + 4eC. ClO2- + 2OH- + 2e-  ClO3- + H2O
D. ClO2- + 2OH-  ClO3- + H2O + 2e-
(basic)
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 Cu2ions migrate toward the Zn.
B. electrons flow toward the Cu and the Zn2ions migrate toward the Cu.
C. electrons flow toward the Zn and the Cu2ions migrate toward the Zn.
D. electrons flow toward the Zn and the Zn2ions 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+ + 2eB. Fe2+ + 2e- Fe
C. 2H2O  O2 + 4H+ + 4eD. O2 + 2H2O + 4e-  4OH46. 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. iodine
B. oxygen
C. hydrogen
D. 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 Ni22eNi
April 1999
37. Which of the following represents the formation of a stronger acid as a result of
oxidation?
A. H2SO3  H2S
B. HClO4  HCl
C. H2SO3  H2SO4
D. HCO3-  H2CO3
38. Chlorine has an oxidation number of 5 in
A. NaClO
B. 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. BrO3B. ClO4-
C. S2O82D. Cr2O72-
41. Consider the following half-reaction:
1 AsH3 + __ H2O  __ H3AsO3 + ? H+ + __eWhen this half-reaction equation is balanced, the coefficient for His
A. 2
B. 3
C. 6
D. 9
42. When a strip of zinc is placed in a 1.0M copper (II) chloride solution,
A. no change occurs.
B. the [Clincreases.
C. the [Cu2increases.
D. the [Zn2increases.
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 IO3B. acidified SO42C. 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 Efor the reaction above is 2.98V. The Efor the oxidation of ethanol is
A. 0.52V
B. 1.23V
C. 1.75V
D. 2.98V
46. Which of the following must be present to produce rust by the corrosion of iron?
A. I only
B. II only
C. I and II only
D. 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. H2O
D. C6H12O6
39. The oxidation number of P in H4P2O7 is
A. -10
B. -5
C. +5
D. +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 + 2OHB. 2CIO- + H2O +2e-  Cl2 + 3OHC. 2CIO- + 2H2O +2e-  Cl2 + 4OHD. 2CIO- + 2H2O Cl2 + 4OH- + 2e42. Which of the following is a spontaneous redox reaction?
A. Ag+ + I-  AgI
B. 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. tin
B. lithium
C. mercury
D. aluminum
45. Consider the following electrochemical cell:
The half-reaction that occurs at the anode is
A. Ni  Ni2+ + 2eB. Ni2+ + 2e-  Ni
C. Cu  Cu2+ + 2eD. Cu2+ + 2e-  Cu
46. Which of the following can be produced by electrolysis from a 1.0M aqueous solution
containing its ion?
A. nickel
B. sodium
C. aluminum
D. magnesium
47. In the electrolysis of molten ZnCl2 using carbon electrodes, the reaction that occurs
at the anode is
A. Zn  Zn2+ + 2eB. Zn 2+ + 2e-  Zn
C. 2Cl-  Cl2 + 2eD. 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. Fe
B. CO
C. CO2
D. Fe2O3
39. Consider the following reaction:
2HNO2 + 2I- + 2H+  2NO + I2 + 2H2O
The oxidation number for each nitrogen atom
A. increases by 1
B. increases by 2
C. decreases by 1
D. 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+ + Cu
D. Ni2+ + 2Ag  2Ag+ + Ni
41. Consider the following redox reaction for a lead-acid storage cell:
Pb + PbO2 + 4H+ + 2SO42-  2PbSO4 + 2H2O
The balanced, reduction half-reaction is
A. Pb + SO42-  PbSO4 + 2eB. Pb + 2H+ + SO42-  PbSO4 + H2O + 2eC. PbO2 + 4H+ + SO42- + 2e-  PbSO4 + 2H2O
D. PbO2 + SO42- + 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 only
B. I and III only
C. II and III only
D. I, II and III
43. At equilibrium, the voltage of the cell above is
A. 1.10 V
B. 0.00 V
C. 0.42 V
D. 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 V
B. 0.40 V
C. 0.40 V
D. 1.12 V
45. Which of the following involves a non-spontaneous redox reaction?
A. fuel cell
B. electroplating
C. redox titration
D. 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 mol
B. 0.060 mol
C. 0.15 mol
D. 0.30 mol
47. What substances are formed at the anode and cathode during electrolysis of molten
sodium 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. 0.54V
B. 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)23- + Br-
39. Consider the following reaction:
TiCl4 + O2  TiO2 + 2Cl2
Each oxygen atom is
A. reduced and loses 2eB. reduced and gains 2eC. oxidized and loses 2eD. oxidized and gains 2e40. When NO2 acts as a reducing agent, a possible product is
A. NO
B. N2O
C. N2O4
D. N2O5
41. Which of the following 1.0M solutions will react spontaneously with lead?
A. KCl
B. CuCl2
C. ZnCl2
D. MgCl2
42. Consider the following redox reaction:
I2 + 2S2O32-  S4O62- + 2IIn 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. 0.10M
B. 0.16M
C. 0.20M
D. 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
B. the
C. the
D. the
Pb electrode, where Pb is oxidized.
Cd electrode, where Cd is oxidized.
Pb electrode, where Pb2+ is reduced.
Cd electrode, where Cd2+ is reduced.
45. The E° value for the reduction of Cd2+ is
A. –0.40V
B. –0.27V
C. +0.14V
D. +0.40V
46. The following reaction occurs in an electrochemical cell:
3Cu2+ + 2Cr  2Cr3+ + 3Cu
The E° for the cell is
A. 0.40V
B. 0.75V
C. 1.08V
D. 2.50V
47. During the corrosion of magnesium, the anode reaction is
A. Mg  Mg2+ + 2eB. Mg2+ + 2e-  Mg
C. 4OH-  O2 + 2H2O + 4eD. O2 + 2H2O + 4e-  4OH48. A molten binary salt, ZnCl2, undergoes electrolysis. The cathode reaction is
A. Zn  Zn2+ + 2eB. 2Cl-  Cl2 + 2eC. Cl2 + 2e-  2ClD. Zn2+ + 2e-  Zn
April 2000
38. Manganese has an oxidation number of +4 in
A. MnO
B. MnO2
C. Mn2O3
D. Mn2O7
39. In which reaction is nitrogen reduced?
A. 2NO + O2  2NO2
B. 4NH3 + 5O2  4NO + 6H2O
C. Cu2+ + 2NO2 + 2H2O  Cu + 4H+ + 2NO3D. 4Zn + 10H+ + NO3-  4Zn2+ + NH4+ + 3H2O
40. An oxidizing agent will cause which of the following changes?
A. PtO2  PtO
B. 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 + 2H2O
B. Ag2O3 + 2H+ + 2e-  2AgO + H2O
C. Ag2O3 + H2O + 2e-  2AgO + 2OHD. Ag2O3 + 2H2O + 4e-  AgO + 4OH44. The concentration of Fe2+ (aq) can be determined by a redox titration using
A. KBr
B. 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.
B.
C.
D.
Ag+ + I2
Pb2+ + Zn
Mg2+ + Ca
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 + 2eB. Mg2+ + 2e-  Mg
C. H2O  ½O2 + 2H+ + 2eD. 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. +4
B. +5
C. +9
D. +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 electrons
B. 4 electrons
C. 6 electrons
D. 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+
The balanced equation for this half-reaction is
(acidic)
A. Bi2O4 + 6H+ + 5e-  BiO+ + 3H2O
B. Bi2O4 + 8H+ + 6e-  2BiO+ + 4H2O
C. Bi2O4 + 4H+ + 2e-  2BiO+ + 2H2O
D. 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. HCl
D. H2O2
45. Consider the following redox reactions:
2Ag+ + Cd  2Ag + Cd2+
3Cd2+ + 2Nb  2Nb3+ + 3Cd
E° = 1.20V
E° =0.70V
What is the E° for Nb3+ + 3e-  Nb?
A. –1.90V
B. –1.10V
C. –0.50V
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 forms
B. Cd gains 2e- and Cd(OH)2 forms
C. NiO2 loses 2e- and Ni(OH)2 forms
D. 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  2MgO
B. 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. Ca
B. Ni
C. Pb
D. 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+ + 2eB. Pb + SO42-  PbSO4 + 2eC. 2H2SO4 + 2Pb + 2e-  2PbSO4 + 2H2O
D. PbO2 + 4H+ + SO42- + 2e-  PbSO4 + 2H2O
43. Consider the following redox reactions:
HClO + I-  HIO + ClE° = +0.49V
HClO + Br-  HBrO + ClE° = +0.15V
The relative strength of the oxidizing agents from strongest to weakest is
A. HIO > HBrO > HClO
B. HClO > HIO > HBrO
C. HBrO >HIO > HClO
D. 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-  H2O
C. 4OH-  O2 + 2H2O + 4eD. H2 + 2OH-  2H2O + 2e-
45. As the cell operates, observations include
46. What is the cell potential, E°, for this cell?
A. 0.08 V
B. 0.26 V
C. 0.60 V
D. 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-  2H2O
D. NaCl + AgNO3  AgCl + NaNO3
39. The oxidation number of each chromium atom in Cr2O72- is
A. +5
B. +6
C. +7
D. +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 Volts
B. –0.42 Volts
C. +0.42 Volts
D. +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 conditions
C. coating with zinc
D. 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. Zn
D. Zn2+
39. When SO42- reacts to form S2O62-, 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 > Rb
B. Ni > Au > Rb
C. Ni > Rb > Au
D. 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. Ca
C. Na
D. 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 volts
B. –0.60 volts
C. +0.04 volts
D. +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 KOH
B. 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  2HI
B. HCl + NH3  NH4Cl
C. 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 > Pd
B. Pd > Ag > Ru
C. Ru > Ag > Pd
D. 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. Al
B. Au
C. Co
D. 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 Volts
B. -0.46 Volts
C. +0.46 Volts
D. +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. Al
B. Cu
C. Al3+
D. Cu2+
39. Bromine has an oxidation number of +3 in
A. KBrO
B. 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 BrB. Zn and Al3+
C. Au and Sn2+
D. I2 and SO4243. What occurs when a piece of Zn is placed in 1.0M Cu(NO3)2?
A. [Cu2+] decreases
B. [Zn2+] decreases
C. [NO3-] increases
D. 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
B. -0.50 Volts
C. +0.50 Volts
D. +1.02 Volts
46. Which of the following does not affect the cell potential?
A. [Ni2+]
B. [Zn2+]
C. temperature
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.
B. sodium and oxygen.
C. hydrogen and iodine.
D. hydrogen and oxygen.
January 2002
38. A reducing agent
A. loses electrons and is reduced.
B. gains electrons and is reduced.
C. loses electrons and is oxidized.
D. gains electrons and is oxidized.
39. Which of the following could be produced by the reduction of NO2?
A. NO
B. N2O4
C. N2O5
D. HNO3
40. Consider the following redox equation:
3NO + SO42- + Fe3+ + 2H2O → FeS + 3NO3- + 4H+
Which of the following is being oxidized?
A. NO
B. Fe3+
C. H2O
D. SO4241. What is the oxidation number of Cr in Cr2O72- ?
A. +6
B. +7
C. +12
D. +14
42. Which of the following represents a spontaneous redox reaction?
A. 2Br- + Hg2+ → Br2 + Hg
B. Cu + Sn4+ → Cu2+ + Sn2+
C. HCl + NaOH → NaCl + H2O
D. AuCl4- + 3Ag → Au + 4Cl- + 3Ag+
43. Which of the following is the balanced half-reaction for
N2O → NH3OH+
(acidic)
A. N2O + 4H+ + 3e- → NH3OH+
B. N2O + 3H+ + H2O → NH3OH+ + 2eC. N2O + 6H+ + H2O → 2NH3OH+ + 4eD. N2O + 6H+ + H2O + 4e- → 2NH3OH+
Use the following diagram to answer questions 44 to 46.
44. Which material could be used as the cathode to produce an E°cell = +0.46 V?
A. Pb
B. Co
C. Ag
D. MnO2
45. In what directions do the electrons and cations move?
Direction of Electrons
Direction of Cations
A.
Toward the cathode
Toward the anode
B.
Toward the cathode
Toward the cathode
C.
Toward the anode
Toward the anode
D.
Toward the anode
Toward the cathode
46. The concentration of Cu2+ in the copper half-cell will
A. increase as Cu loses electrons and is reduced.
B. increase as Cu loses electrons and is oxidized.
C. decrease as Cu gains electrons and is reduced.
D. decrease as Cu gains electrons and is oxidized.
47. Which of the following metals could be used to cathodically protect iron?
A. tin
B. lead
C. zinc
D. copper
48. Which of the following is formed at the anode during the electrolysis of 1.0M KF?
A. K
B. F2
C. H2
D. O2
April 2002
38. Which of the following describes a strong oxidizing agent?
A. a substance which loses electrons readily
B. a substance which gains electrons readily
C. a substance which has a large increase in oxidation number
D. a substance which has a small increase in oxidation number
39. Consider the following unbalanced redox reacton:
Sn2+ + MnO4- → Sn4+ + Mn2+
Which of the following describes the change in Sn2+ ?
A. loses electrons and is reduced
B. gains electrons and is reduced
C. loses electrons and is oxidized
D. gains electrons and is oxidized
40. A solution containing Pd2+ reacts spontaneously with Ga to produce Pd and Ga3+.
However, a solution containing Pd2+ does not react with Pt. The metals, in order of
Increasing strength as reducing agents, are
A. Pt < Pd < Ga
B. Pt < Ga < Pd
C. Ga < Pt < Pd
D. Ga < Pd < Pt
41. Which of the following can act as an oxidizing agent, but not as a reducing agent?
A. Cr
B. ClC. Cu+
D. Na+
42. Solid copper forms spontaneously in the following reaction:
V + Cu2+ → Cu + V2+
Based on this observation, Cu2+ is a
A. weaker reducing agent than V2+
B. weaker oxidizing agent than V2+
C. stronger reducing agent than V2+
D. stronger oxidizing agent than V2+
43. Which of the following could be used to determine the [Fe2+] by a redox titration?
A. I2
B. ClC. Cu2+
D. MnO4- (acidified)
Use the following diagram to answer questions 44, 45 and 46.
44. What happens to the lead electrode?
A. It loses mass as it is reduced.
B. It gains mass as it is reduced.
C. It loses mass as it is oxidized.
D. It gains mass as it is oxidized.
45. As the cell operates, what happens to the ions in the salt bridge?
A. K+ and NO3- will both migrate toward the Pb half-cell.
B. K+ and NO3- will both migrate toward the Cu half-cell.
C. K+ will migrate toward the Cu half-cell and NO3- will migrate toward the Pb half-cell.
D. K+ will migrate toward the Pb half-cell and NO3- will migrate toward the Cu half-cell.
46. What is the initial cell voltage?
A. +0.02 V
B. +0.21 V
C. +0.28 V
D. +0.47 V
47. Consider the following:
I.
II.
III.
Electrolysis of water
Electroplating of copper
Rusting of iron
Which of the above involve non-spontaneous redox reactions?
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
48. A copper spoon was electroplated with silver. Which of the following reactions
occurred at the cathode during electroplating?
A. Ag → Ag+ + eB. Ag+ + e- → Ag
C. Cu → Cu2+ + 2eD. Cu2+ + 2e- → Cu
June 2002
38. Which of the following is the strongest reducing agent?
A. H2S
B. H2O
C. H2Se
D. H2Te
39. Consider the following unbalanced half-reaction:
H2SeO3 → Se
The oxidation number of Se
A. increases as it undergoes oxidation.
B. increases as it undergoes reduction.
C. decreases as it undergoes oxidation.
D. decreases as it undergoes reduction.
40. Which of the following will react spontaneously with Br2 but not with I2?
A. FB. Cr2+
C. Fe2+
D. Mn2+
41. Consider the following:
Sn4+ + 2Cl- → Sn2+ + Cl2
What is true for this reaction?
A. E°cell = +1.51 V and it is spontaneous.
B. E°cell = +1.21 V and it is spontaneous.
C. E°cell = -1.21 V and it is non-spontaneous.
D. E°cell = -1.51 V and it is non-spontaneous.
42. What is the function of the salt bridge in an electrochemical cell?
A. It provides a path for electrons.
B. It maintains electrical neutrality in each half cell.
C. It allows the anode to become positively charged.
D. It allows the cathode to become negatively charged.
Use the following diagram to answer questions 43, 44 and 45.
43. In the above electrochemical cell, how do the mass of the anode and the [Ag+]
change as the cell operates?
Mass of the Anode
[Ag+]
A.
Decreases
Increases
B.
Increases
Increases
C.
Decreases
Decreases
D.
No change
decreases
44. What is the overall cell reaction?
A. 2Ag + Sn2+ → Sn + 2Ag+
B. 2Ag + Sn → Sn2+ + 2Ag+
C. 2Ag+ + Sn2+ → Sn + 2Ag
D. 2Ag+ + Sn → Sn2+ + 2Ag
45. What is the value of E° for the cell?
A. -0.94 V
B. -0.66 V
C. +0.66 V
D. +0.94 V
46. Consider the following equation:
Cd2+ + 2I- ⇄ Cd + I2
E°cell = -0.94 V
What is E° for the reduction of Cd2+ ?
A. -0.40 V
B. -0.14 V
C. +0.14 V
D. +0.40 V
47. Which of the following describes an operating electrochemical cell?
A.
B.
C.
D.
E°
Positive
Negative
Positive
negative
Type of Reaction
Spontaneous
Spontaneous
Non-spontaneous
Non-spontaneous
Direction of Electron Flow
adnoe to cathode
Cathode to anode
Anode to cathode
Cathode to anode
48. A copper spoon is plated with silver in an electrolytic cell.
What is the reaction at the anode?
A. Ag → Ag+ + eB. Ag+ + e- → Ag
C. Cu → Cu2+ + 2eD. Cu2+ + 2e- → Cu
August 2002
38. An oxidizing agent is
A. reduced as it loses electrons.
B. reduced as it gains electrons.
C. oxidized as it loses electrons.
D. oxidized as it gains electrons.
39. Consider the following spontaneous reaction:
Ga3+ + 3Rb → 3Rb+ + Ga
What happens in this reaction?
A. Rb is reduced.
B. Rb gains electrons.
C. Ga3+ loses electrons.
D. Ga3+ acts as an oxidizing agent.
40. What is the oxidation number of S in S2O62- ?
A. +3
B. +5
C. +6
D. +7
41. Which of the following is the weakest oxidizing agnet?
A. Cl2
B. Al3+
C. Sn2+
D. acidified Cr2O7242. Which of the following could react spontaneously with Ag metal?
A. ClB. Fe2+
C. acidified SO42D. acidified NO343. Which of the following could be titrated using acidified MnO4- ions?
A. Na+
B. IO3C. SO42D. H2O2
Use the following diagram to answer questions 44 and 45.
44. What happens to the zinc electrode?
A. Mass increases as it is reduced.
B. Mass decreases as it is reduced.
C. Mass increases as it is oxidized.
D. Mass decreases as it is oxidized.
45. Calculate the E for the above cell.
A.-0.42 V
B. 0.91 V
C. 1.10 V
D. 1.30 V
46. What happens to iron as it corrodes?
A. It loses electrons and is reduced.
B. It gains electrons and is reduced.
C. It loses electrons and is oxidized.
D. It gains electrons and is oxidized.
Use the following diagram to answer questions 47 and 48.
47. What reaction occurs at the cathode?
A. 2I- → I2 + 2eB. Cu2+ + 2e- → Cu
C. H2O → 1/2O2 + 2H+ + 2eD. 2H2O + 2e- → H2 + 2OH-
48. What happens to the [I-] in the operating cell?
A. [I-] increases overall.
B. [I-] decreases overall.
C. [I-] remains constant overall.
D. [I-] decreases near the anode and increases near the cathode.
January 2003
38. Consider the following equation:
16H+ + 2MnO4- + 5C2O42- → 10CO2 + 2Mn2+ + 8H2O
Identify the chemical species which is reduced.
A. H+
B. Mn2+
C. MnO4D. C2O4239. Consider the following equation:
H3AsO4 + 4Zn + 8H+ → AsH3 + 4Zn2+ + 4H2O
Which of the following is correct?
A. Oxygen is reduced.
B. Arsenic is oxidized.
C. Zinc is the oxidizing agent
D. The reaction is a redox reaction.
40. What is the oxidation number of iron in magnetite, Fe3O4?
A. +4/3
B. +2
C. +8/3
C. +3
41. Consider the following spontaneous reactions:
3Cd2+ + 2Np → 3Cd + 2Np3+
Cd + Pd2+ → Pd + Cd2+
Np3+ + Ce → Np + Ce3+
Which is the strongest oxidizing agent?
A. Cd2+
B. Ce3+
C. Np3+
D. Pd2+
42. The volumetric analysis of hydrogen peroxide is often carried out by titrating with
aqueous KMnO4 in an acidic solution. The unbalanced formula equation for the
reaction is:
H2O2 + KMnO4 + H2SO4 → K2SO4 + MnSO4 + H2O + O2
Which of the following is the correct set of balancing coefficients?
A. 1,1,1,1,1,1,1
B. 1,2,3,1,2,4,3
C. 2,5,3,2,1,8,5
D. 5,2,3,1,2,8,5
43. Which of the following would not be founding all electrochemical cells?
A. ions
B. an anode
C. a cathode
D. two beakers
Use the following diagram to answer questions 44 and 45.
44. As this cell operates, the cations move towards the
A. Pb electrode and the electrode gains mass.
B. Pd electrode and the electrode loses mass.
C. Zn electrode and the electrode gains mass.
D. Zn electrode and the electrode loses mass.
45. As the cell operates, the electrons flow towards the
A. Zn electrode and the cell voltage increases over time.
B. Pb electrode and the cell voltage decreases over time.
C. Zn electrode and the cell voltage decreases over time.
D. Pb electrode and the cell voltage remains constant over time.
46. Consider the following electrochemical cell:
What is the E° for this cell?
A. -1.62 V
B. -1.10 V
C. +1.10 V
D. +1.62 V
47. An aqueous solution of CuSO4 is electrolyzed using copper electrodes. Which of
the following would correctly describe the changes in the mass of each electrode
and the [Cu2+] in solution?
Mass of Anode
increases
increases
decreases
decreases
A.
B.
C.
D.
Mass of Cathode
increases
decreases
increases
decreases
[Cu2+]
increases
stays the same
stays the same
increases
48. Which of the following are produced at the anode and cathode in the elctrolysis of
aqueous potassium sulfate using carbon electrodes?
A.
B.
C.
D.
Anode
Potassium
Hydrogen
Oxygen
Sulfur
Cathode
Oxygen
Oxygen
Hydrogen
Potassium
April 2003
38. The equation for the decomposition of nitrous acid is
3HNO2 → 2NO + HNO3 + H2O
Which of the following is correct?
A. This is a redox reaction.
B. This is an acid-base reaction.
C. This is a reduction half equation.
D. This is an oxidation half equation.
39. An equation for the rusting of iron is shown below:
4Fe + 3O2 → 2Fe2O3
Which of the following is false?
A. This is a redox reaction.
B. O2 is the oxidizing agent.
C. Metallic iron is reduced to Fe3+.
D. Metallic iron is the reducing agent.
40. In which of the following chemical changes will there be an oxidation number change
of +3?
A. Cr3+ → Cr2+
B. ClO- → ClO2C. Cr3+ → Cr2O72D. Mn2+ → MnO441. Which of the following ions can be reduced by Pb(s) under standard conditions?
A. Cu+
B. Cr3+
C. Sn2+
D. Ca2+
42. Consider the following equation for the combustion of ethane:
2C2H6 + 7O2 → 4CO2 + 6H2O
The change in oxidation number for carbon is equivalent to
A. 1 electron lost.
B. 7 electrons lost.
C. 1 electron gained.
D. 7 electrons gained.
43. Consider the diagram below:
Identify the cathode half reaction.
A. H2 → 2H+ + 2eB. 2H+ + 2e- → H2
C. Au3+ + 3e- → Au
D. Co2+ + 2e- → Co
44. As a standard Zn / Ag electrochemical cell operates, in which direction do anions
move and how does the mass of the cathode change?
Anion Direction
Mass of Cathode
A.
Towards Zn electrode
Increases
B.
Towards Ag electrode
Increases
C.
Towards Zn electrode
Decreases
D.
Towards Ag electrode
Decreases
45. What is the standard cell potential for the following reaction:
2Cr(s) + 3Cu2+ → 2Cr3+ + 3Cu(s)
A. -1.08 V
B. +0.40 V
C. +1.08 V
D. +2.50 V
46. Consider the following:
2Cr2+ + Tl3+ → 2Cr3+ + Tl+
E° = +1.19 V
Identify the standard potential for the half-cell reaction:
Tl+ → Tl3+ + 2eA. -0.78 V
B. +1.60 V
C. +0.78 V
D. +1.19 V
47. The electrolysis of aqueous Rb2SO4 solution using carbon electrodes produces
changes in the solution around the electrodes. How will the pH change around the
anode and the cathode?
pH around the Anode
pH around the Cathode
A.
Increase
Increase
B.
Decrease
Decrease
C.
Increase
Decrease
D.
decrease
increase
48. The same amount of electricity (same number of moles of electrons) is used to carry
out the electrolysis of PdCl2(aq) and AgNO3(aq) solutions in separate cells. The
masses of Pd and Ag produced were measured and compared. Which of the
following is true about the mass Pd produced?
A. The mass of Pd produced is not related to the mass of Ag.
B. The mass of Pd produced is approximately half that of Ag.
C. The mass of Pd produced is approximately twice that of Ag.
D. The mass of Pd produced is approximately the same as that of Ag.
June 2003
38. Which of the following represents an oxidation?
A. 2H+ + S → H2S
B. 2SO42- → S2O82C. Na+ + Cl- → NaCl
D. SO2 + H2O → 2H+ + SO3239. Identify the oxidation number for manganese in MnO4-.
A. -7
B. +7
C. +8
D. +9
40. Which of the following is more difficult to reduce than the H+(aq) ion?
A. I2
B. Ag+
C. Zn2+
D. Cu2+
41. Nitric oxide (NO) can be prepard by the oxidation of Cu with NO3- in acidic
solution. Copper is oxidized to Cu2+ and NO3- is reduced to NO. Which of the
following equations correctly describes this process?
A. Cu + NO3- + 4H+ → Cu2+ + NO + 2H2O
B. Cu + NO3- + 2H+ → Cu2+ + NO2 + H2O
C. Cu + 4NO3- + 4H+ → Cu2+ + 2NO2 + 2H2O
D. 3Cu + 2NO3- + 8H+ → 3Cu2+ + 2NO + 4H2O
42. Acidified potassium permanganate (KMnO4) solution is often used in redox
titrations. Permanganate reacts with Sn2+ as follows:
2MNO4- + 5Sn2+ +16H+ → 2MN2+ + 5Sn4+ + 8H2O
A 10.0mL solution containing Sn2+ is titrated with 19.3 mL of 0.10 M KMnO4.
What is the [Sn2+] in the solution?
A. 0.077 M
B. 0.19 M
C. 0.25 M
D. 0.48 M
43. Given the following half-cell reactions:
PbO2 + 4H+ + SO42- + 2e- ⇄ PdSO4 + 2H2O
E° = +1.69 V
PbSO4 + 2e ⇄ Pb +
E° = -0.36 V
-
SO42-
Which of the following best describes the overall reaction and the standard cell voltage
in a lead acid storage battery?
A. Pb + 2H2O → PbO2 + 4H+ + 4eB. PbO2 + 4H+ + 4e- → Pb + 2H2O
C. Pb + PbO2 + 2SO42- + 4H+ → 2PbSO4 + 2H2O
D. 2PbSO4 + 2H2O → Pb + PbO2 + 2SO42- + 4H+
44. Consider the following electrochemical cell:
What is the anode half-reation?
E°cell = +1.33
E°cell = +1.33
E°cell = +2.05
E°cell = +2.05
A. Ag → Ag+ + eB. Ag+ + e- → Ag
C. Zn → Zn2+ + 2eD. Zn2+ + 2e- → Zn
45. Consider the following cell:
What is the value of the standard cell potential?
A. -0.76 V
B. +0.76 V
C. +2.12 V
D. +2.26 V
46. Two separate reactions involved in the refining of copper ore are:
Reaction I
2Cu2S + 3O2 → 2Cu2O + 2SO2
Reaction II
Cu2S + 2Cu2O → 6Cu + SO2
What happens to the copper ions during this process?
A. They are reduced in Reaction I.
B. They are reduced in Reaction II.
C. They are oxidized in Reaction I.
D. They are oxidized in Reaction II.
47. Why is aluminum a good choice for the manufacture of outdoor structures?
A. Pure aluminum is easily reduced.
B. Pure aluminum is not easily oxidized.
C. Pure aluminum is easily reduced, but forms a protective coating.
D. Pure aluminum is easily oxidized, but forms a protective coating.
48. Which of the following are produced at the anode and the cathode during the
electrolysis of aqueous calcium iodide using carbon electrodes?
A.
B.
C.
D.
Anode
Iodine
Hydrogen
Oxygen
Iodine
Cathode
Calcium
Oxygen
Hydrogen
Hydrogen
August 2003
38. Which equation represents a redox reaction?
A. C + O2 → CO2
B. NH3 + HCl → NH4Cl
C. 2CrO42- + 2H+ → Cr2O72- + H2O
D. CaCO3 + 2HCl → CaCl2 + CO2 + H2O
39. What is a typical characteristic of a strong oxidizing agent?
A. It is readily oxidized.
B. It easily loses electrons.
C. It has a negative oxidation number.
D. It has a positive reduction potential.
40. When U3O8 (pitchblende) is dissolved in nitric acid, it changes into UO2(NO3)2
(uranyl nitrate). What is the change in oxidation number for uranium?
41. The metals Hg, Cd, Ga and Pd react as follows:
3Pd2+ + 2Ga → 2Ga3+ + 3Pd
Cd + Ga3+ → no reaction
Hg2+ + Pd → Pd2+ + Hg
Which of the following metals is the strongest reducing agent?
A. Pd
B. Ga
C. Cd
D. Hg
42. Which of the following metals can be oxidized by 1.0M Fe2+ ?
A. Sn
B. Co
C. Cr
D. Ag
Use the following diagram to answer questions 43 to 45.
43. What is the equation for the half-reaction that occurs at the cathode?
A. Ag → Ag+ + eB. Ag+ + e- → Ag
C. Zn → Zn2+ + 2eD. Zn2+ + 2e- → Zn
44. What happens to the mass of each electrode as the cell operates?
A. Ag(s) increases, Zn(s) increases
B. Ag(s) decreases, Zn(s) decreases
C. Ag(s) decreases, Zn(s) increases
D. Ag(s) increases, Zn(s) decreases
45. Which of the following is correct?
A.
B.
C.
D.
Electrons Flow
Towards
Anions
Move Towards
Zn
Zn
Ag
Ag
Zn
Ag
Zn
Ag
46. Consider the following diagram:
Identify the anode reaction for the cell shown in the diagram.
A. H2 → 2H+ + 2eB. Co → Co2+ + 2eC. Co2+ + 2e- → Co
D. MnO4- + 8H+ + 5e- → Mn2+ + 4H2O
47. Consider the following cell:
What is the initial cell voltage?
A. +0.87 V
B. +0.61 V
C. +0.54 V
D. +0.28 V
48. Which of the following are produced at the anode and the cathode in the
electrolysis of molten lithium chloride using platinum inert electrodes?
A.
B.
C.
D.
Anode
oxygen
hydrogen
chlorine
lithium
Cathode
hydrogen
oxygen
lithium
chlorine
Electrochemistry Multiple Choices Answers
January 1999
B
37
A
38
D
39
A
40
A
41
A
42
B
43
D
44
D
45
C
46
C
47
C
48
April 1999
C
37
C
38
B
39
C
40
C
41
D
42
A
43
B
44
C
45
C
46
D
47
B
48
June 1999
C
37
A
38
C
39
B
40
C
41
B
42
B
43
C
44
A
45
A
46
C
47
C
48
August 1999
D
37
B
38
C
39
C
40
C
41
D
42
B
43
B
44
B
45
C
46
D
47
D
48
January 2000
B
38
B
39
D
40
B
41
C
42
C
43
C
44
A
45
C
46
A
47
D
48
April 2000
B
38
D
39
D
40
A
41
D
42
C
43
D
44
D
45
B
46
D
47
D
48
June 2000
D
38
B
39
A
40
C
41
A
42
C
43
D
44
B
45
D
46
B
47
A
48
August 2000
A
37
B
38
A
39
C
40
A
41
D
42
D
43
D
44
B
45
C
46
D
47
D
48
January 2001
A
38
B
39
D
40
C
41
C
42
D
43
B
44
D
45
D
46
C
47
D
48
April 2001
C
38
B
39
D
40
C
41
D
42
B
43
A
44
D
45
A
46
D
47
B
48
June 2001
A
38
C
39
D
40
A
41
C
42
B
43
A
44
C
45
B
46
D
47
A
48
August 2001
D
38
B
39
A
40
A
41
A
42
A
43
C
44
C
45
D
46
A
47
C
48
January 2002
C
38
A
39
A
40
A
41
D
42
D
43
C
44
B
45
B
46
C
47
D
48
April 2002
B
38
C
39
A
40
D
41
D
42
D
43
C
44
C
45
D
46
A
47
B
48
June 2002
D
38
D
39
C
40
C
41
B
42
C
43
D
44
D
45
A
46
A
47
A
48
August 2002
B
38
D
39
B
40
B
41
D
42
D
43
D
44
C
45
C
46
B
47
B
48
January 2003
C
38
D
39
C
40
D
41
D
42
D
43
A
44
B
45
D
46
C
47
C
48
April 2003
A
38
C
39
C
40
A
41
B
42
B
43
A
44
C
45
A
46
D
47
B
48
June 2003
B
38
B
39
C
40
D
41
D
42
C
43
C
44
B
45
B
46
D
47
D
48
August 2003
A
38
D
39
B
40
B
41
C
42
B
43
D
44
C
45
B
46
B
47
C
48