Question 1

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

Accepted Answer

It maintains electrical neutrality by allowing the migration of ions between the two half-cells.

Question 2

In the galvanic cell depicted, which electrode acts as the cathode?

Accepted Answer

The platinum electrode in the H2/H3O+ half-cell.

Question 3

What is the direction of electron flow in the external circuit of the cell shown?

Accepted Answer

From the iron electrode to the platinum electrode.

Question 4

Which half-reaction occurs at the cathode in the cell shown?

Accepted Answer

Fe3+(aq) + e– → Fe2+(aq)

Question 5

What is the role of the platinum electrode in the right half-cell?

Accepted Answer

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

Question 6

If the voltmeter reads +0.77 V, what does this indicate about the spontaneity of the cell reaction?

Accepted Answer

The cell reaction is spontaneous in the forward direction.

Question 7

Which species is being oxidized in the cell shown?

Accepted Answer

H2(g)

Question 8

What is the balanced half-reaction for the oxidation process occurring at the anode in the cell?

Accepted Answer

$$\mathrm{H}_2(g) \rightarrow 2\mathrm{H}^+(aq) + 2e^-$$

Question 9

If the concentration of Fe3+ in the left half-cell is increased, what effect will this have on the cell potential?

Accepted Answer

The cell potential will increase.

Question 10

Which equation can be used to calculate the cell potential under non-standard conditions?

Accepted Answer

$$E_{cell} = E^\circ_{cell} - \frac{0.0592}{n} \log Q$$

Question 11

What would happen if the salt bridge were removed from the cell?

Accepted Answer

The cell would quickly stop functioning due to charge buildup.

Question 12

Which of the following statements about the cell diagram is correct?

Accepted Answer

The anode is the iron electrode and the cathode is the platinum electrode.

Question 13

If the hydrogen gas pressure is decreased below 1 atm in the right half-cell, what effect will this have on the cell potential?

Accepted Answer

The cell potential will decrease.

Question 14

Which of the following is the correct shorthand notation for the cell shown?

Accepted Answer

$$\mathrm{Fe}(s) | \mathrm{Fe}^{3+}(aq), \mathrm{Fe}^{2+}(aq) || \mathrm{H}^+(aq) | \mathrm{H}_2(g) | \mathrm{Pt}$$

Question 15

What is the purpose of using a chemically inert platinum electrode in the right half-cell?

Accepted Answer

To provide a surface for electron transfer without participating in the reaction.

Question 16

If the Fe2+ concentration in the left half-cell decreases, what happens to the cell potential?

Accepted Answer

The cell potential decreases.

Question 17

Which of the following best describes the overall cell reaction?

Accepted Answer

$$\mathrm{H}_2(g) + 2\mathrm{Fe}^{3+}(aq) \rightarrow 2\mathrm{Fe}^{2+}(aq) + 2\mathrm{H}^+(aq)$$

Question 18

Which ion migrates through the salt bridge toward the left half-cell as the cell operates?

Accepted Answer

Cations

Question 19

If the cell is operated for a long time, what will eventually happen to the concentrations of Fe3+ and Fe2+ in the left half-cell?

Accepted Answer

Fe3+ concentration will increase and Fe2+ concentration will decrease.

General Chemistry Exam IV Study Guidance: Kinetics & Electrochemistry

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