Problem: You synthesize a new molecule X in the lab. You construct an electrochemical cell in which one cell contains a copper metal electrode and dissolved copper sulfate, and the other cell contains an inert platinum electrode and an aqueous solution of your new molecule X and its soluble chloride salt XCl. The concentration of both solutions is 1 M. When you hook up the cell you find that your compound is spontaneously oxidized. You measure the potential of this cell and find it to be 0.2 V. Based on this information what is the potential for the reactionX+(aq) + 1e− → X(aq)A. +0.14 VB. +0.54 VC. +0.84 VD. -0.06 VE. +0.20 V

FREE Expert Solution

We’re being asked to determine the potential for the reaction:

X+(aq) + 1e → X(aq)


Recall  that:

↓ E° → oxidation

Loss Electrons → Oxidation

 ↑ E° → reduction

Gain Electrons → Reduction


Since it was mentioned that X was spontaneously oxidized, we know from the X is the anode and Cu2+ is the cathode.

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Problem Details

You synthesize a new molecule X in the lab. You construct an electrochemical cell in which one cell contains a copper metal electrode and dissolved copper sulfate, and the other cell contains an inert platinum electrode and an aqueous solution of your new molecule X and its soluble chloride salt XCl. The concentration of both solutions is 1 M. When you hook up the cell you find that your compound is spontaneously oxidized. You measure the potential of this cell and find it to be 0.2 V. Based on this information what is the potential for the reaction

X+(aq) + 1e → X(aq)

A. +0.14 V

B. +0.54 V

C. +0.84 V

D. -0.06 V

E. +0.20 V

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