AP - Advanced Placement Electrochemistry 1

Question 1

Calculate ΔG° for the reaction in the Zn-Cu galvanic cell (E°cell = 1.10 V, n = 2, F = 96,485 C/mol e⁻).

Accepted Answer

−212 kJ/mol

Answer

−106 kJ/mol

Answer

−424 kJ/mol

Answer

+212 kJ/mol

Question 2

A concentration cell is constructed: Cu(s) | Cu²⁺(0.0100 M) || Cu²⁺(1.00 M) | Cu(s). What is the cell potential at 25°C? (n = 2)

Accepted Answer

0.0592 V

Answer

0.0296 V

Answer

0.118 V

Answer

0.00 V

Question 3

For a spontaneous electrochemical reaction at 25°C involving n moles of electrons transferred, which expression correctly gives the equilibrium constant K from the standard cell potential E°?

Accepted Answer

log K = nE° / 0.0592

Answer

log K = E° / (n × 0.0592)

Answer

log K = nFE° / R

Answer

ln K = nE° / 0.0592

Question 4

During the electrolysis of aqueous sodium chloride (brine), what is the product formed at the cathode?

Accepted Answer

H₂(g)

Answer

Cl₂(g)

Answer

Na(s)

Answer

O₂(g)

Question 5

Given standard reduction potentials — Cu²⁺/Cu = +0.34 V, Ag⁺/Ag = +0.80 V, Zn²⁺/Zn = −0.76 V, Fe²⁺/Fe = −0.44 V — which metal will NOT spontaneously dissolve in 1.0 M HCl to produce H₂(g)? (E°(H⁺/H₂) = 0.00 V)

Accepted Answer

Cu

Answer

Zn

Answer

Fe

Answer

Both Zn and Fe

Question 6

How many seconds are required to deposit 2.16 g of silver (MM = 107.87 g/mol) from an AgNO₃ solution using a constant current of 2.00 A? (Ag⁺ + e⁻ → Ag; F = 96,485 C/mol e⁻)

Accepted Answer

966 s

Answer

483 s

Answer

1932 s

Answer

241 s