AP Electrochemistry 2

Question 1

Calculate the standard cell potential (E°cell) for the galvanic cell: Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s). Given: E°(Zn²⁺/Zn) = −0.76 V and E°(Cu²⁺/Cu) = +0.34 V.

Accepted Answer

+1.10 V

Answer

+0.42 V

Answer

−1.10 V

Answer

+0.76 V

Question 2

Using the Nernst equation, what is the cell potential at 25°C for the Zn-Cu cell when [Zn²⁺] = 2.0 M and [Cu²⁺] = 0.010 M? (E°cell = 1.10 V, n = 2)

Accepted Answer

1.04 V

Answer

1.10 V

Answer

1.16 V

Answer

1.07 V

Question 3

In the electrolysis of molten NaCl, which species is produced at each electrode?

Accepted Answer

Cathode: Na metal; Anode: Cl₂ gas

Answer

Cathode: Cl₂ gas; Anode: Na metal

Answer

Cathode: H₂ gas; Anode: O₂ gas

Answer

Both electrodes produce NaCl

Question 4

How many grams of copper (MM = 63.55 g/mol) are deposited during the electrolysis of a CuSO₄ solution when a current of 2.50 A flows for 30.0 minutes? (F = 96,485 C/mol e⁻)

Accepted Answer

1.48 g

Answer

2.96 g

Answer

0.740 g

Answer

0.370 g

Question 5

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

Accepted Answer

It allows ions to flow between half-cells to maintain electrical neutrality without mixing the solutions

Answer

It transfers electrons directly between the anode and cathode

Answer

It prevents any ion migration so the two half-cell solutions remain pure

Answer

It provides additional electromotive force to the cell

Question 6

For the half-reaction: Fe³⁺ + e⁻ → Fe²⁺, E° = +0.77 V. What is the value of ΔG° for this process when n = 1? (F = 96,485 C/mol)

Accepted Answer

−74.3 kJ/mol

Answer

+74.3 kJ/mol

Answer

−148.6 kJ/mol

Answer

+148.6 kJ/mol

Calculate the standard cell potential (E°cell) for the galvanic cell: Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s).Given: E°(Zn²⁺/Zn) = −0.76 V and E°(Cu²⁺/Cu) = +0.34 V.

Calculate the standard cell potential (E°cell) for the galvanic cell: Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s).
Given: E°(Zn²⁺/Zn) = −0.76 V and E°(Cu²⁺/Cu) = +0.34 V.