Oxidation Reduction Reactions and Electrochemistry MCQ

Reduction-Oxidation Reactions and Electrochemistry MCQ In recitation, you studied the electrochemistry involved in the &...

Reduction-Oxidation Reactions and Electrochemistry MCQ




  1. In recitation, you studied the electrochemistry involved in the "fruit clock". If an orange is used to power the fruit clock, which of the following statements is TRUE?
    1. Free electrons flow through the orange to maintain electrical neutrality.
    2. The orange allows the Zn2+ and Cu2+ ions produced in the reaction to mix thereby maintaining electrical neutrality.
    3. The orange functions as the anode.
    4. The orange functions as the salt bridge by maintaining electrical neutrality.
    5. The acids present in the orange are oxidized at the anode to produce hydrogen gas.
  2. Which of the following reactions IS a reduction-oxidation reaction?

    1. formation of N2 in automobile airbags: 2NaN3(s) --> 2Na(l) + 3N2(g)
    2. combustion of propane in a gas grill: C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g)
    3. decomposition of hydrogen peroxide (H2O2) by light: 2H2O2(aq) --> 2H2O(l) + O2(g)
    4. All of these are reduction-oxidation reactions.
    5. None of these are reduction-oxidation reactions.

  1. Which of the following metals could be used successfully to galvanize iron?
    1. Ni
    2. Cu
    3. Sn
    4. Co
    5. Mn
  1. Calculate the standard cell potential (in V) for the following reaction at 25oC.

2Cr(s) + 3Ni2+(aq) --> 2Cr3+(aq) + 3Ni(s)
  1. The layer of zinc on a piece of galvanized iron can be removed by placing it in a concentrated solution of acid. Calculate the standard cell potential (in V) for this reaction.
  2. A beaker contains a small amount of gold dust (Au(s)). Which of the following aqueous solutions, when added to the beaker, would dissolve the gold dust (i.e., convert Au(s) to Au3+(aq))?
    1. Cr2O72- (acidic solution)
    2. H2O2 (acidic solution)
    3. Br2
    4. Zn2+
    5. Al3+
  3. Which of the following statements best describes what will happen when liquid bromine (Br2) is poured into a beaker containing aluminum metal?
    1. Br2 will be reduced; Al will be oxidized
    2. Br2 will be oxidized; Al will be reduced
    3. Br2 will function as the reducing agent; Al will function as the oxidizing agent
    4. A reaction will not occur.
    5. It is impossible to tell.
  1. Consider the following galvanic cell reaction at 25oC,
4Cr2+(aq) + O2(g) + 4H3O+(aq) --> 4Cr3+(aq) + 6H2O(l)
Which of the following statements best describes what would happen to the cell potential if the concentration of Cr2+ is increased?
    1. The cell potential would become less positive.
    2. The cell potential would become more positive.
    3. The cell potential would remain the same.
    4. It is impossible to tell.
  1. Which of the following half-reactions is involved in the STANDARD HYDROGEN ELECTRODE?
    1. Pt2+(aq) + 2e- --> Pt(s)
    2. 2H3O+(aq) + 2e- --> 2H2O(l) + H2(g)
    3. H2O2(aq) + 2H3O+(aq) + 2e- --> 4H2O(l)
    4. O2(g) + 2H2O(l) + 4e- --> 4OH-(aq)
    5. None of the above.
  1. A concentration cell containing aqueous solutions of Cu(NO3)2 and solid copper metal is constructed so that the Cu2+ ion concentration in the cathode half-cell is 0.66 M. Calculate the concentration of the Cu2+ ion in the anode half-cell if the cell potential for the concentration cell at 25oC is 0.034 V.
  2. Consider a galvanic cell based on the following overall reaction,
Fe(s) + 2Ag+(aq) --> Fe2+(aq) + 2Ag(s)
Calculate the cell potential (in V) for this reaction at 25oC when the concentration of Ag+ ions is 0.050 M and the concentration of Fe2+ ions is 1.50 M.
  1. Which of the following metal ions will plate out on a piece of galvanized iron which has NOT had the layer of Zn metal removed?
    1. Cu2+
    2. Au3+
    3. Ni2+
    4. All of these.
    5. None of these.
  2. Which of the following best explains why concentration cells must be run under non-standard conditions in order for them to do electrical work?
    1. A concentration cell can only do electrical work when either NH3 or NaOH is added to one of the half-cells.
    2. A concentration cell cannot do electrical work at 25oC.
    3. The change in free energy for a concentration cell is always negative under standard conditions.
    4. A concentration cell has a cell potential equal to zero under standard conditions.
    5. A concentration cell can only do electrical work when the cell is run under standard conditions.
  1. Which of the following statements about a salt bridge in a voltaic cell is TRUE?
    1. Free electrons flow through the salt bridge to maintain electrical neutrality in the two half-cells.
    2. The salt bridge allows the ions present in the two half-cells to mix extensively.
    3. The wire must be connected directly to the salt bridge in order for the salt bridge to be able to maintain electrical neutrality in the two half-cells.
    4. In some cases, a salt bridge functions as the anode.
    5. Ions from the electrolyte in the salt bridge flow into each half-cell to maintain electrical neutrality.
  1. Which of the following reactions can be used to construct a voltaic cell?
    1. H3O+(aq) + OH-(aq) <==> 2H2O(l)
    2. HF(g) + H2O(l) <==> H3O+(aq) + F-(aq)
    3. Cu2+(aq) + 4F-(aq) <==> CuF42-(aq)
    4. O2(g) + 4H3O+(aq) + 4I-(aq) <==> 2I2(aq) + 6H2O(l)
    5. 2NO2(g, nitrogen dioxide) <==> N2O4(g, dinitrogen tetroxide)
  1. Consider the following standard reduction potentials,
half reaction
Eo, V
Fe3+(aq) + e- <==> Fe2+(aq)
0.77
H2O2(aq) + 2e- <==> 2OH-(aq)
0.88
  1. For the voltaic cell reaction below, calculate the Fe2+ concentration (in M) that would be needed to produce a cell potential equal to 0.16 V at 25oC when (OH-) = 0.10 M, (Fe3+) = 0.50 M and (H2O2) = 0.35 M.
  2. 2Fe2+(aq) + H2O2(aq) --> 2Fe3+(aq) + 2OH-(aq)
  3. Consider the following standard reduction potentials,
half reaction
Eo, V
Ni2+(aq) + 2e- <==> Ni(s)
-0.23
Co2+(aq) + 2e- <==> Co(s)
-0.28
Fe2+(aq) + 2e- <==> Fe(s)
-0.41
Cr3+(aq) + 3e- <==> Cr(s)
-0.74
Mn2+(aq) + 2e- <==> Mn(s)
-1.03
  1. which of the following metals could be used successfully to galvanize steel?
    1. Ni only
    2. Ni and Co
    3. Fe only
    4. Mn only
    5. Mn and Cr
  2. Consider the following standard reduction potentials,
half reaction
Eo, V
Ag+(aq) + e- <==> Ag(s)
0.800
AgI(s) + e- <==> Ag(s) + I-(aq)
-0.164
  1. Calculate the value of the solubility product equilibrium constant, Ksp, at 25oC for silver iodide (AgI).
  2. AgI(s) <==> Ag+(aq) + I-(aq)
  3. Which of the following is TRUE for an operating voltaic cell?
    1. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG > 0 ; E = 0
    2. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG < 0 ; E < 0
    3. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG = 0 ; E > 0
    4. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG = 0 ; E = 0
    5. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG < 0 ; E > 0
  4. Consider the following standard reduction potentials,
half reaction
Eo, V
Cu2+(aq) + 2e- <==> Cu(s)
0.34
MnO4-(aq) + 2H2O(l) + 3e- <==> MnO2(s) + 4OH-(aq)
0.59
O2(g) + 2H3O+(aq) + 2e- <==> H2O2(aq) + 2H2O(l)
0.68
  1. and the following redox reactions,
27.i.     H2O2(aq) + 2H2O(l) + Cu2+(aq)  <==>  O2<(g) + 2H3O+(aq) + Cu(s)
28. 
29.ii.    2MnO4-(aq) + 4H2O(l) + 3Cu(s)  <==>  3Cu2+(aq) + 2MnO2(s) + 8OH-(aq)
30. 
31.iii.   2MnO4-(aq) + 10H2O(l) + 3H2O2(aq)  <==>  3O2(g) + 6H3O+(aq) + 2MnO2(s) + 8OH-(aq)
  1. Which of the redox reactions above will be spontaneous under standard conditions?
    1. i only
    2. ii only
    3. i and iii
    4. ii and iii
    5. None of these.
  2. In recitation, you saw that silver tarnish (Ag2S(s)) can be converted to silver metal (Ag(s)) by placing the tarnished silver piece in a dilute solution of baking soda contained in an aluminum pan. The following half-reactions are thought to be involved,
Ag2S(s) + 2H3O+(aq) + 2e- <==> 2Ag(s) + H2S(g) + 2H2O(l)
Al3+(aq) + 3e- <==> Al(s)
Which of the following statements is TRUE?
    1. As the silver piece is being cleaned, H3O+ ions are produced and H2S gas is consumed.
    2. It is necessary that the silver piece and the aluminum pan touch so that electrons can be transferred.
    3. As the silver piece is being cleaned, Al3+ ions in the solution are reduced to Al metal.
    4. The silver piece being cleaned functions as the anode.
    5. All of the above are TRUE.
  1. Calculate the cell potential (in V) at 25oC for a copper concentration cell in which the Cu2+ concentration in one half-cell is equal to 0.050 M and the Cu2+ concentration in the other half-cell is equal to 1.5 M. Note: the number of moles of electrons transferred is equal to 2.
  2. Which of the following is a correctly balanced oxidation/reduction reaction.
    1. Fe2+ + Au3+ <=> Fe3+ + Au
    2. 2 Fe2+ + Au3+ <=> 2 Fe3+ + Au
    3. Fe2+ + 3 Au3+ <=> Fe3+ + 3 Au
    4. 3 Fe2+ + Au3+ <=> 3 Fe3+ + Au
    5. The correct response is not given.
  1. In acid solution, dichromate ion oxidizes ferrous iron to ferric iron as illustrated in the partial equation:
Fe2+ + Cr2O72- <=> Fe3+ + Cr3+
When this equation is balanced, the right side of the equation will be as follows:
    1. <=> Fe3+ + 2 Cr3+ + 7 H2O
    2. <=> 6 Fe3+ + 2 Cr3+ + 7 H2O
    3. <=> 3 Fe3+ + 2 Cr3+ + 7 H2O
    4. <=> Fe3+ + 2 Cr3+ + H2O
    5. The correct response is not given.
  1. You have observed all of the reactions listed below. Which of these reactions IS a reduction-oxidation reaction?
    1. HCl(aq) + H2O(l) --> H3O+(aq) + Cl-(aq)
    2. Fe2O3(s, iron oxide) + 2Al(s) --> 2Fe(s) + Al2O3(s, aluminum oxide)
    3. Cu2+(aq) + 4NH3(aq) --> Cu(NH3)42+(aq)
    4. NH4NO3(s, ammonium nitrate) --> NH4+(aq) + NO3-(aq)
    5. None of these is a reduction-oxidation reaction.
  1. In an electrochemical process called "electrolysis", H2 gas and O2 gas can be obtained by passing an electric current through liquid water,
2H2O(l) --> 2H2(g) + O2(g)
Which species is the OXIDIZING AGENT and which species is the REDUCING AGENT in this reaction, respectively?
    1. H2O(l) ; H2(g)
    2. O2(g) ; H2O(l)
    3. H2O(l) ; H2O(l)
    4. O2(g) ; H2(g)
    5. H2(g) ; H2O(l)
  1. In recitation, you saw that silver tarnish (Ag2S(s)) can be converted to silver metal (Ag(s)) by placing the tarnished silver piece in a dilute solution of baking soda contained in an aluminum pan. The following half-reactions are involved,
Ag2S(s) + 2H3O+(aq) + 2e- --> 2Ag(s) + H2S(g) + 2H2O(l)
Al3+(aq) + 3e- --> Al(s)
Which of the following is the correct overall balanced equation for the reaction?
    1. Ag2S + 2H3O+ + Al --> 2Ag + H2S + Al3+ + 2H2O
    2. 6Ag + 3H2S + 6H2O + 2Al3+ --> 2Al + 3Ag2S + 6H3O+
    3. Ag2S + Al --> Ag + Al3+
    4. 2Al + 3Ag2S + 6H3O+ --> 6Ag + 3H2S + 6H2O + 2Al3+
    5. Ag2S + 2H3O+ + Al --> 2Ag + H2S + 2H2O + Al3+ + e-
  1. Which of the following statements about porous disks in voltaic cells is TRUE?
    1. Free electrons flow through the porous disk to maintain electrical neutrality in the two half-cells.
    2. Ions present in the two half-cells flow through the porous disk to maintain electrical neutrality in both half-cells.
    3. A porous disk contains a strong electrolyte like potassium chloride (KCl).
    4. The wire must be connected directly to the porous disk in order for the porous disk to be able to maintain electrical neutrality in the two half-cells.
    5. In some cases, a porous disk functions as the cathode.
  1. In the Standard Hydrogen Electrode, a platinum wire is used as the electrode. Consider the following standard reduction potentials,
half reaction
Eo, V
Zn2+(aq) + 2e- --> Zn(s)
-0.76
2H3O+(aq) + 2e- --> 2H2O(l) + H2(g)
0.00
Pt2+(aq) + 2e- --> Pt(s)
1.20
  1. Which of the following statements best describes what would happen if the platinum wire in the Standard Hydrogen Electrode were replaced with a zinc wire? Note: assume that this is the only change made to the half-cell.
    1. Zinc ion in the solution would be reduced; the mass of the zinc electrode would increase.
    2. The pH of the solution would decrease.
    3. The zinc electrode would be oxidized; the mass of the zinc electrode would decrease.
    4. This change would have no effect - the Standard Hydrogen Electrode would continue to function properly.
    5. It is impossible to tell.
  2. In recitation, you examined a diagram of a voltaic cell constructed from zinc and copper in which a tube containing a porous disk and a solution of KCl was placed in each half-cell (recall, the two tubes were not connected). Which of the following statements best describes why this cell has a cell potential of 0.00 V?
    1. The sum of the zinc and copper half-cell potentials is equal to 0.00 V.
    2. Electrical neutrality cannot be maintained in the half-cells and the KCl tubes.
    3. All voltaic cells which use zinc in one of the half-cells have a cell potential of 0.00 V.
    4. The tubes needed to contain a weak electrolyte, like AgCl, in order for the cell to function.
    5. There was not enough information given to solve the problem.
  1. Which of the following statements best describes what will happen when magnesium metal is added to an aqueous solution containing 1.0 M ferric ion (Fe3+) at 25oC?
half reaction
Eo, V
Mg2+(aq) + 2e- --> Mg(s)
-2.375
Fe3+(aq) + 3e- --> Fe(s)
-0.036
    1. Mg(s) will be oxidized; Fe3+(aq) will be reduced; the standard cell potential will be 2.339 V.
    2. Mg(s) will be oxidized; Fe3+(aq) will be reduced; the standard cell potential will be -2.339 V.
    3. Fe3+(aq) will be oxidized; Mg(s) will be reduced; the standard cell potential will be -2.339 V.
    4. Fe3+(aq) will be oxidized; Mg(s) will be reduced; the standard cell potential will be 2.339 V.
    5. There is not enough information given to answer the question.
  1. In recitation, you explored the electrochemistry of the "fruit clock". Which of the following statements best describes why the clock functions best when citrus fruits (i.e., lemons, oranges, limes, etc.) are used?
    1. Citrus fruits work best because they are often brightly colored.
    2. Only fruits and vegetables that grow on trees can be used to power the fruit clock.
    3. Citrus fruits contain very high concentrations of copper ion.
    4. Acid is a product in one of the half-reactions involved.
    5. Acid is a reactant in one of the half-reactions involved.
  1. Suppose you have been given the task of selecting a metal to be used as the sacrificial anode for the cathodic protection of a buried iron fuel tank. Considering the following standard reduction potentials,
half reaction
Eo, V
Pd2+(aq) + 2e- --> Pd(s)
0.99
Ag+(aq) + e- --> Ag(s)
0.80
Cu2+(aq) + 2e- --> Cu(s)
0.34
Ni2+(aq) + 2e- --> Ni(s)
-0.23
Fe2+(aq) + 2e- --> Fe(s)
-0.41
  1. which of the following metals could be used as the sacrificial anode in this application?
    1. Pd
    2. Ag
    3. Cu
    4. Ni
    5. None of these.
  2. In lecture, one area of current research in electrochemistry was described: the development of improved batteries for use in electric cars. Which of the following properties of batteries are researchers currently trying to improve?
    1. range (the number of miles that can be driven before the batteries must be recharged)
    2. cost
    3. lifetime (the number of times the batteries can be recharged before they must be replaced)
    4. recharge time (the time required to fully recharge the batteries)
    5. Researchers are currently trying to improve all of the above.
  1. Use the Standard Reduction Potentials given below to calculate Kf for Zn(NH3)42+ at 25oC.
Zn2+(aq) + 4NH3(aq) <==> Zn(NH3)42+(aq), Kf = ??
half reaction
Eo, V
Zn(NH3)42+(aq) + 2e- <==> Zn(s) + 4NH3(aq)
-1.04
Zn2+(aq) + 2e- <==> Zn(s)
-0.76
  1. The cell potential for the electrochemical reaction shown below depends upon the Cl- and Cu2+ concentrations. Calculate the cell potential (in V) at 25oC if [Cu2+] = 3.5 M and [Cl-] = 1.7 M. Note: the number of moles of electrons transported in this reaction is equal to 2.
Cu2+(aq) + 2Cl-(aq) + 2Ag(s) --> Cu(s) + 2AgCl(s), Eo = 0.12 V
  1. Consider the following standard reduction potentials,
half reaction
Eo, V
I3-(aq) + 2e- --> 3I-(aq)
0.53
Cr3+(aq) + e- --> Cr2+(aq)
-0.41
  1. Calculate http://www.chem.purdue.edu/gchelp/116exams/delta.gifGo (in kJ) for the following reaction at 25oC.
  2. Cr2+(aq) + I3-(aq) --> Cr3+(aq) + I-(aq)
  3. In which of the following reactions does the oxidation number of the sulfur atom NOT CHANGE?
    1. 3S2- + 8H+ + 2NO3- (nitrate ion) --> 2NO + 3S + 4H2O
    2. 2SO2 (sulfur dioxide) + O2 --> 2SO3 (sulfur trioxide)
    3. 2H2S + 3O2 --> 2SO2 (sulfur dioxide) + 2H2O
    4. S8 + 8O2 --> 8SO2 (sulfur dioxide)
    5. SO2 (sulfur dioxide) + H2O --> H2SO3 (sulfurous acid)
  4. Which of the following reactions IS a reduction-oxidation reaction?
    1. NH3(aq) + H2O(l) --> NH4+(aq) + OH-(aq)
    2. Cu2+(aq) + 4NH3(aq) --> Cu(NH3)42+(aq)
    3. AgF(s) --> Ag+(aq) + F-(aq)
    4. 2Cu+(aq) --> Cu2+(aq) + Cu(s)
    5. 2NO2(g, nitrogen dioxide) --> N2O4(g, dinitrogen tetroxide)
  1. Which of the following statements explains why a definition of standard state conditions is needed in electrochemistry?
    1. Cell potentials vary with concentration.
    2. Cell potentials vary with temperature.
    3. Cell potentials vary with partial pressures of gases.
    4. Responses (a) and (c) are correct.
    5. Responses (a), (b) and (c) are all correct.
  1. Consider the following reaction and standard cell potential,
Ni2+(aq) + 6NH3(aq) --> Ni(NH3)62+(aq), Eo = +0.25 V
Which of the following best describes what would happen in a solution that initially contains 1.0 M Ni2+, 0.01 M NH3 and 6.0 M Ni(NH3)62+ at 25oC? (Assume that the number of moles of electrons transported in this reaction is equal to 2.)
    1. The concentrations of both Ni2+ and NH3 would decrease and the concentration of Ni(NH3)62+ would increase.
    2. The concentrations of both Ni2+ and NH3 would increase and the concentration of Ni(NH3)62+ would decrease.
    3. The concentration of Ni(NH3)62+ would decrease, the concentration of NH3 would increase and the concentration of Ni2+ would remain the same.
    4. The concentrations of Ni2+, NH3 and Ni(NH3)62+ would all remain the same.
    5. It is impossible to tell.
  1. Consider the following standard reduction potentials,
half reaction
Eo, V
Ca2+ + 2e- --> Ca
-2.76
Pb2+ + 2e- --> Pb
-0.13
Cu2+ + 2e- --> Cu
+0.34
Hg22+ + 2e- --> Hg
+0.80
Pt2+ + 2e- --> Pt
+1.20
  1. Which of the following metals is the strongest REDUCING AGENT?
    1. Ca
    2. Pb
    3. Cu
    4. Hg
    5. Pt
  2. Consider the following standard reduction potentials,
half reaction
Eo, V
Fe2+ + 2e- --> Fe
-0.4090
Ag+ + e- --> Ag
0.7996
O2 + 2H2O + 4e- --> 4OH-
+0.4010
  1. Which of the following statements best describes what would happen if a block of silver metal were connected to a buried iron pipe via a wire (i.e., as in a cathodic protection process).
    1. The silver metal would corrode, a current would be produced in the wire, and O2 would be reduced on the surface of the iron pipe.
    2. The silver metal would corrode, a current would be produced in the wire, and Fe2+ would be reduced on the surface of the iron pipe.
    3. The iron pipe would corrode, a current would be produced in the wire, and Ag+ would be reduced on the surface of the silver metal.
    4. The iron pipe would corrode, no current would be produced in the wire, and O2 would be reduced on the surface of the iron pipe.
    5. Neither the iron pipe nor the silver metal would be oxidized but O2 would be reduced.
  2. Consider the following reduction-oxidation reaction,
Zn(s) + Cu2+(aq) --> Cu(s) + Zn2+(aq), Eo = +1.10 V
When the components of the two half-reactions involved in this reaction are correctly separated, this reaction can be used to do electrical work and the change in internal energy of the system decreases. Which of the following statements best describes what will happen if Zn(s) is added to a solution containing Cu2+(aq) at constant volume at 25oC?
    1. The reaction will occur and the temperature of the solution will increase.
    2. The reaction will occur and the temperature of the solution will decrease.
    3. The reaction will occur and the temperature of the solution will remain the same.
    4. The reaction will not occur and the temperature of the solution will remain the same.
    5. The reaction will not occur but the temperature of the solution will increase.
  1. Using the following standard reduction potentials,
half reaction
Eo, V
Cl2 + 2e- --> 2Cl-
+1.36
Cr3+ + 3e- --> Cr
-0.74
  1. calculate http://www.chem.purdue.edu/gchelp/116exams/delta.gifGo (in kJ) for the reaction,
  2. 3Cl2 + 2Cr --> 6Cl- + 2Cr3+
  3. Use the following information to answer the next four (4) questions.
  4. A galvanic cell is constructed from a half cell containing a solid copper electrode in 1.0 M Cu(NO3)2 solution and a half cell containing a solid aluminum electrode in 1.0 M Al(NO3)3 solution at standard conditions. The half cells are linked by an external circuit and by a KCl salt bridge.
  5. The balanced overall (net) cell reaction for a spontaneous process is:
    1. Cu(s) + Al3+(aq) --> Cu2+(aq) + Al(s)
    2. 3 Cu(s) + 2 Al3+(aq) --> 3 Cu2+(aq) + 2 Al(s)
    3. 3 Cu2+(aq) + 2 Al(s) --> 3 Cu(s) + 2 Al3+(aq)
    4. Cu2+(aq) + Al(s) --> Cu(s) + Al3+(aq)
    5. The reaction is not spontaneous.
  6. Which of the following statements is TRUE about this cell?
    1. The aluminum electrode is the anode; the copper electrode is the cathode.
    2. The electrons flow from the copper electrode to the aluminum electrode.
    3. The cell diagram is |Cu solid|Cu2+, 1.0 M|salt bridge|Al solid|Al3+, 1.0 M|
    4. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG is greater than zero.
    5. http://www.chem.purdue.edu/gchelp/116exams/delta.gifS is the driving force of this reaction.
  1. This cell generates a standard potential of:
    1. +1.32 V
    2. -2.00 V
    3. -1.32 V
    4. +2.00 V
    5. The cell is at equilibrium.
  1. An expression for the equilibrium constant of this reaction at 25oC is:
    1. e205
    2. e298
    3. e467
    4. e831
    5. e965
  1. You have installed a new hot water heater in your house, and you notice that the iron tank has a large metal bar bolted to it on the inside. You conclude that this bar is a sacrificial anode and that it could be made of:
    1. Ag
    2. Ni
    3. Pb
    4. Sn
    5. Mg
  1. We used copper and zinc electrodes stuck in an apple to run a small clock. Which of the following statements must be TRUE?
    1. The zinc strip was the anode.
    2. The apple was the salt bridge.
    3. Ecell > 0.
    4. http://www.chem.purdue.edu/gchelp/116exams/delta.gifG < 0.
    5. All of these statements are true.



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Advanced Chemistry: Oxidation Reduction Reactions and Electrochemistry MCQ
Oxidation Reduction Reactions and Electrochemistry MCQ
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Advanced Chemistry
https://www.advancedchemistry.in/2019/12/oxidation-reduction-electrochemistry-mcq.html
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