Electrochemistry | Practice Test / Quiz / MCQs

1. Which of the following choices best explains why the reaction represented above generates electricity in a galvanic cell?

Cl2 loses electrons more easily than Br2.Cl2 is a stronger oxidizing agent than Br2.Br2 is more stable than Cl2.Br atoms have more electrons than Cl atoms.Cl? is more stable than Br?.

3. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. Which of the following is true regarding the HCl half-cell?

The reduction of H+ to H2 is neither spontaneous nor non-spontaneous.The reduction of H+ and oxidation of H2 are at equilibrium.The E° value of 0 V for the hydrogen half-cell is arbitrary.All electrochemical cells use a hydrogen half-cell.It is used to measure the reduction potential of Zn2+ because the reduction potential has a measured value of zero volts.

4. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. Which of the following changes to the voltage, if any, would result from increasing the concentration of ZnSO4?

Increased voltage, the value of Q will fall below 1 and the log term in the Nernst equation will become more negative.Decreased voltage, the value of Q will fall below 1 and the log term in the Nernst equation will become more negative.Decreased voltage, the increased concentration of Zn2+ will inhibit the oxidation of Zn(s).No change, the voltage of the cell is determined only by the standard reduction potentials of the electrodes.Increased voltage, the reaction becomes more favorable as the concentration of Zn+ increases.

5. A 0.1-M solution of H3PO4 is a better conductor of electricity than a 0.1-M solution of NaCl. Which of the following best explains this observation?

NaCl has a lower molar mass than H3PO4.NaCl is less soluble than H3PO4.Fewer moles of ions are present in the NaCl solution than in the same volume of an Na3PO4 solution.H3PO4 is weakly acidic, which increases the flow of charge through a solution.H3PO4 dissociates to produce particles of a larger size than NaCl.

6. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. The salt bridge is filled with a saturated solution of KNO3. Processes that occur at the salt bridge include which of the following? I. K+ moves into the anode half-cell. II. K+ moves into the cathode half-cell. III. NO3− moves into the anode half-cell. IV. NO3− moves into the cathode half-cell.

I and IV onlyI onlyI, II, III, and IVIII onlyII and III only

7. Iron nails are often electroplated (galvanized) with zinc. Which of the following is true regarding this process (E° of Zn2+ → Zn(s) = –0.76 V, E° of Fe2+ → Fe(s) = –0.44 V)?

The galvanization process produces an alloy of Zn and Fe that is stronger and more resistant to oxidation than Fe alone.The galvanization process is spontaneous, thereby reducing the energy cost of producing nails.Zn serves as a sacrificial anode for Fe.Zn serves as an airtight seal preventing the electrons from iron from reacting with oxygen.The oxidation of Zn allows the reduction of Fe2+ to proceed spontaneously.

8. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. The salt bridge is filled with a saturated solution of KNO3. Processes that occur at the salt bridge include which of the following? I. K+ moves into the anode half-cell. II. K+ moves into the cathode half-cell. III. NO3− moves into the anode half-cell. IV. NO3− moves into the cathode half-cell.

II and III onlyIII onlyI onlyI, II, III, and IVI and IV only

9. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. Which of the following is true regarding the standard free energy change (ΔG°) of the cell?

It is negative because the oxidation of Zn is spontaneous.It has a value of zero because the reaction is at equilibrium.It is negative because the sum of the standard reduction potentials of Zn2+ and H+ is –0.76 V.It is positive because the reduction of hydrogen ions is spontaneous.It is negative because the standard reduction potential of Zn2+ is negative.

10. Which of the following statements is/are true regarding the reaction above? I. Cu(s) acts as an oxidizing agent. II. H+(aq) gets reduced. III. The oxidation state of nitrogen changes from +5 to +2.

III onlyII and III onlyI, II, and IIIII onlyI only

11. Which of the following statements is/are true regarding the reaction above? I. Cu(s) acts as an oxidizing agent. II. H+(aq) gets reduced. III. The oxidation state of nitrogen changes from +5 to +2.

I, II, and IIIII and III onlyI onlyIII onlyII only

12. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. Which of the following changes to the voltage, if any, would result from increasing the concentration of ZnSO4?

Increased voltage, the reaction becomes more favorable as the concentration of Zn+ increases.No change, the voltage of the cell is determined only by the standard reduction potentials of the electrodes.Increased voltage, the value of Q will fall below 1 and the log term in the Nernst equation will become more negative.Decreased voltage, the increased concentration of Zn2+ will inhibit the oxidation of Zn(s).Decreased voltage, the value of Q will fall below 1 and the log term in the Nernst equation will become more negative.

14. The photodecomposition of permanganate is shown above. As this reaction proceeds in the forward direction and the reaction species are considered from left to right, the oxidation number of Mn changes from:

+1 to +2 and +2+7 to +2 and +2+5 to +2 and +2+7 to +6 and +4+5 to +6 and +4

15. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. Which of the following correctly identifies and justifies which species, Zn or Zn2+, has the highest ionization energy?

Zn, electrons have a greater affinity for pure metals.Zn2+, it has a greater electron-to-proton ratio.Zn2+, it has a larger radius.Zn, it has a greater electron to proton ratio.Zn2+, it has a greater effective nuclear charge.

16. A galvanic cell made of two half-cells. In one half-cell, a Zn electrode is bathed in a 1.0 M ZnSO4 solution. The other cell contains a 1 M HCl solution and a hydrogen electrode. Which of the following is true regarding the standard free energy change (ΔG°) of the cell?

It is negative because the oxidation of Zn is spontaneous.It is positive because the reduction of hydrogen ions is spontaneous.It is negative because the standard reduction potential of Zn2+ is negative.It has a value of zero because the reaction is at equilibrium.It is negative because the sum of the standard reduction potentials of Zn2+ and H+ is –0.76 V.

17. Which of the following correctly relates the quantities needed for the conversion of chemical energy into electrical energy in a galvanic cell?

The difference between the voltages of the two half-cells.The product of the gas constant and the voltage divided by the total charge passed through the cell.The sum of the E° cell of the two half-cells.The product of cell voltage and the natural log (ln) of K, the equilibrium constant for the redox reaction.The product of the cell voltage and the total charge passed through the cell.

18. Iron nails are often electroplated (galvanized) with zinc. Which of the following is true regarding this process (E° of Zn2+ → Zn(s) = –0.76 V, E° of Fe2+ → Fe(s) = –0.44 V)?

Zn serves as a sacrificial anode for Fe.The galvanization process is spontaneous, thereby reducing the energy cost of producing nails.Zn serves as an airtight seal preventing the electrons from iron from reacting with oxygen.The galvanization process produces an alloy of Zn and Fe that is stronger and more resistant to oxidation than Fe alone.The oxidation of Zn allows the reduction of Fe2+ to proceed spontaneously.

19 Questions

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19 Questions

❤ If you liked Fatskills, consider supporting us by checking out The Life Manuals You Never Got.

About | Explore | User Guide | Topics | Subjects | Doubt Solver | Career Aptitude Test | Answers | Free Tools | OSHA Basics Quiz | What Should We Know? Privacy | Terms |

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All trademarks, logos and brand names are the property of their respective owners. All company, product and service names used in this website are for identification purposes only. Use of these names, trademarks and brands does not imply endorsement.

About | Explore | User Guide | Topics | Subjects | Doubt Solver | Career Aptitude Test | Answers | Free Tools | OSHA Basics Quiz | What Should We Know?
Privacy | Terms |

Without work one finishes nothing. - Ralph Waldo Emerson
© 2026 Fatskills.com