Question 1

Why is it necessary to separate the oxidizing agent from the reducing agent in a galvanic cell?

Accepted Answer

To prevent the direct transfer of electrons, which would release energy as heat instead of electrical energy.

Question 2

Which of the following best describes the function of a salt bridge in a galvanic cell?

Accepted Answer

It allows ions to flow between half-cells to maintain electrical neutrality.

Question 3

In the reaction $$\mathrm{Zn(s) + $$CuSO_4$$(aq) \rightarrow $$ZnSO_4$$(aq) + Cu(s)}$$, which species is oxidized?

Accepted Answer

Zn(s)

Question 4

What is the correct half-reaction for the reduction process in a zinc-copper galvanic cell?

Accepted Answer

$$\mathrm{Cu$$^{2+}$$(aq) + 2e^- \rightarrow Cu(s)}$$

Question 5

Which observation would indicate that the zinc electrode is acting as the anode in a galvanic cell?

Accepted Answer

The zinc electrode decreases in mass over time.

Question 6

What is the direction of electron flow in a functioning zinc-copper galvanic cell?

Accepted Answer

From the zinc electrode (anode) to the copper electrode (cathode) through the wire.

Question 7

Which of the following is a correct line notation for a galvanic cell with zinc and copper electrodes?

Accepted Answer

$$\mathrm{Zn(s) | Zn$$^{2+}$$(aq) || Cu$$^{2+}$$(aq) | Cu(s)}$$

Question 8

A galvanic cell is constructed using magnesium and nickel electrodes. Which metal acts as the anode?

Accepted Answer

Magnesium

Question 9

What is the role of an inert electrode in a galvanic cell?

Accepted Answer

It provides a surface for the redox reaction without participating in the reaction.

Question 10

Which of the following best explains why a galvanic cell stops producing current if the salt bridge is removed?

Accepted Answer

Charge buildup in the half-cells prevents further electron flow.

Question 11

In a galvanic cell, which direction do anions move through the salt bridge?

Accepted Answer

Toward the anode

Question 12

Given the reaction $$\mathrm{8H^+(aq) + $$MnO_4$$^-(aq) + 5Fe$$^{2+}$$(aq) \rightarrow Mn$$^{2+}$$(aq) + 5Fe$$^{3+}$$(aq) + 4H_2O(l)}$$, which species is the stronger oxidizing agent?

Accepted Answer

$$\mathrm{$$MnO_4$$^-(aq)}$$

Question 13

Which of the following would you expect to observe as a galvanic cell operates with a magnesium anode and an iron cathode?

Accepted Answer

The magnesium electrode decreases in mass and the iron electrode increases in mass.

Question 14

What is the net ionic equation for a galvanic cell with magnesium and copper electrodes?

Accepted Answer

$$\mathrm{Mg(s) + Cu$$^{2+}$$(aq) \rightarrow Mg$$^{2+}$$(aq) + Cu(s)}$$

Question 15

Which of the following is a requirement for the solution used in a salt bridge?

Accepted Answer

It must contain ions that do not react with the electrodes or the electrolytes.

Question 16

In a galvanic cell, what is the function of the cathode?

Accepted Answer

It is where reduction occurs.

Question 17

A student constructs a galvanic cell using a strip of magnesium in magnesium sulfate and a strip of nickel in nickel(II) sulfate. Which of the following is the correct net ionic equation for the cell reaction?

Accepted Answer

$$\mathrm{Mg(s) + Ni$$^{2+}$$(aq) \rightarrow Mg$$^{2+}$$(aq) + Ni(s)}$$

Question 18

Which of the following best explains why tap water can be used in a galvanic cell but distilled water cannot?

Accepted Answer

Tap water contains ions that allow it to conduct electricity, while distilled water does not.

Lesson 10.1: Galvanic Cells: Transforming Chemical Energy into Electrical Energy

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