Evaluating Cell Reaction and Spontaneity

Very Hard General Chemistry Electrochemistry

Consider a galvanic cell constructed using a copper(II) sulfate solution and a zinc sulfate solution. The standard reduction potentials for the half reactions are as follows:

Cu²⁺ + 2e^- → Cu(s) ; E^° = +0.34 V

Zn²⁺ + 2e^- → Zn(s) ; E^° = -0.76 V

Based on these reduction potentials, which of the following statements is TRUE regarding the overall cell reaction and its characteristics in terms of spontaneous behavior and current flow direction?

The spontaneous reaction is Zn(s) + Cu2+ → Zn2+ + Cu(s) with a positive cell potential.

The spontaneous reaction is Cu(s) + Zn2+ → Cu2+ + Zn(s) with a cell potential of +0.34 V.

The net cell potential is negative, indicating a non-spontaneous reaction between the two half-cells.

The spontaneous reaction is solely dictated by the higher reduction potential of Cu2+, irrespective of the Zn electrode.

Hint

Submitted2.4K

Correct2.2K

% Correct90%