Chemistry

Problem

A galvanic cell is assembled from two half-cells separated by a salt bridge and connected by an external wire. The cell is represented symbolically as

Zn(\text{s}) \;|\; Zn^{2+}\,(1.0\,\text{M}) \;||\; Cu^{2+}\,(1.0\,\text{M}) \;|\; Cu(\text{s})

Assume all solutions are at

25\,^{\circ}\text{C}

and

1.0\,\text{M}

concentration. Answer the following. a. Part 1: Identify which electrode is the anode and which is the cathode in this cell. Justify your assignment in terms of the chemical changes occurring at each electrode. b. Part 2: State the direction in which electrons move through the external wire. Express your answer using the names of the metals involved. c. Part 3: Describe the directions of migration for the cations and anions within the salt bridge as the cell operates. Explain how this migration maintains electrical neutrality in each half-cell. d. Part 4: Predict whether the mass of each metal electrode increases or decreases as the cell produces current. Provide a chemical explanation for each prediction.

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