Question 1

A copper strip is placed in a solution of silver nitrate (AgNO$$_3). $$After some time, silver metal forms on the copper strip and the solution turns blue. Which species is oxidized in this reaction?

Accepted Answer

Cu(s)

Question 2

In the reaction between copper metal and silver nitrate solution, how many moles of electrons are transferred per mole of copper reacted?

Accepted Answer

2 moles

Question 3

Which component of an electrochemical cell is responsible for balancing the charge by allowing ion flow between the two half-cells?

Accepted Answer

Salt bridge

Question 4

A Galvanic cell is constructed with a copper electrode in 1.0 M Cu$$^{2+}$$ and an aluminum electrode in 1.0 M Al$$^{3+}. $$Using the standard reduction potentials, what is the standard cell potential $$E^\circ_{cell}$$?

Accepted Answer

$$2.00 V$$

Question 5

For the cell in the previous question, what is the value of $$\Delta G^\circ$$ for the overall reaction? (Use $$F = 96,485 C/$$mol e$$^-$$ and $$n = 6)$$

Accepted Answer

$$-1,158 kJ$$

Question 6

In a Galvanic cell, which direction do electrons flow?

Accepted Answer

From anode to cathode

Question 7

Which way do cations in the salt bridge flow in a Galvanic cell?

Accepted Answer

Toward the cathode

Question 8

Why does the standard cell potential $$E^\circ_{cell}$$ not change when the overall reaction is multiplied by a factor (e.g., doubled)?

Accepted Answer

Because $$E^\circ_{cell} is an $$intensive property and does not depend on the amount of substance

Question 9

Which of the following reactions is spontaneous under standard conditions? Use the reduction potentials: $$\mathrm{Cu$$^{2+}$$ + 2e^- \rightarrow Cu} (0.34 V$$), $$\mathrm{2H^+ + 2e^- \rightarrow H_2$} (0.00 V).$$

Accepted Answer

$$\mathrm{Cu$$^{2+}$$ + H_2$(g) \rightarrow Cu(s) + 2H^+}$$

Question 10

A piece of iron metal is placed in a solution of copper(II) sulfate. Will copper metal deposit on the iron? Use the reduction potentials: $$\mathrm{Cu$$^{2+}$$ + 2e^- \rightarrow Cu} (0.34 V$$), $$\mathrm{Fe$$^{2+}$$ + 2e^- \rightarrow Fe} (-0.44 V).$$

Accepted Answer

Yes, because $$E^\circ_{cell} \u003e 0$$

Question 11

Which of the following is the correct line notation for a Galvanic cell with a zinc anode and a silver cathode?

Accepted Answer

Zn | Zn$$^{2+}$$ || Ag$$^+$$ | Ag

Question 12

Which of the following is the strongest oxidizing agent based on the standard reduction potentials provided?

Accepted Answer

F$$_2$$

Question 13

Which of the following can oxidize aluminum but cannot oxidize copper? Use the reduction potentials: $$\mathrm{Cu$$^{2+}$$ + 2e^- \rightarrow Cu} (0.34 V$$), $$\mathrm{Al$$^{3+}$$ + 3e^- \rightarrow Al} (-1.66 V$$), $$\mathrm{2H^+ + 2e^- \rightarrow H_2$} (0.00 V).$$

Accepted Answer

H$$^+$$

Question 14

Does Ag(s) dissolve in HNO$$_3(aq$$)? Use the reduction potentials: $$\mathrm{NO_3$^- + 4H^+ + 3e^- \rightarrow NO_2$ + 2H_2O} (0.96 V$$), $$\mathrm{Ag^+ + e^- \rightarrow Ag} (0.80 V).$$

Accepted Answer

Yes, because NO$$_3^- is a $$strong enough oxidizing agent

Question 15

Which equation correctly relates the cell potential under nonstandard conditions to the standard cell potential?

Accepted Answer

$$E_{cell} = E^\circ_{cell} - \frac{0.059}{n} \log Q$$

Question 16

In a concentration cell with Ag electrodes, one compartment contains 0.1 M Ag$$^+$$ and the other 1.0 M Ag$$^+. $$What is the cell potential at 25$$^\circC$$?

Accepted Answer

$$0.059 V$$

Question 17

How long will it take to plate out 10.0 grams of Ni(s) from a Ni$$^{2+}$$ solution with a current of 100. A? (Ni molar mass = 58.7 g/mol, $$n = 2)$$

Accepted Answer

$$1,700 s$$

Question 18

A nonspontaneous redox reaction can be forced to occur by:

Accepted Answer

Applying an external voltage (electrolysis)

Question 19

Which of the following best describes the role of the anode in an electrochemical cell?

Accepted Answer

Site of oxidation

Electrochemistry: Galvanic Cells, Electrolysis, and Cell Potentials

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