Question

Two voltaic cells are to be joined so that one will run the other as an electrolytic cell. In the first cell, one half-cell has Au foil in 1.00 M Au(NO₃)₃, and the other half-cell has a Cr bar in 1.00 M Cr(NO₃)₃. In the second cell, one half-cell has a Co bar in 1.00 M Co(NO₃)₂, and the other half-cell has a Zn bar in 1.00 M Zn(NO₃)₂.(d) Which metal ion is being reduced in each cell?

Answer 1

Au³⁺ metal ion is reduced in the Au/Cr cell and Co²⁺ metal ion is reduced in the Co/Zr cell

What is a voltaic cell?

A voltaic cell is a cell that generates electricity by a spontaneous redox reaction.

It is an electrochemical cell, also known as a galvanic cell and  

Electrical energy is created by converting chemical energy.

Examples of voltaic cells include the dry cell, nickel-cadmium cell, lead storage cell, and fuel cells.

The half-cell reactions for each cell are given by

$Au^{3+}(aq) + 3e^- \rightarrow Au(s)$ ; E° = 1.50 V

$Cr^{3+}(aq) + 3e^- \rightarrow Cr(s)$ ; E° = –0.74 V

$Co^{2+}(aq) + 2e^- \rightarrow Co(s)$ ; E° = –0.28 V

$Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ E° = –0.76 V

Thus, Au³⁺ is reduced in the Au/Cr cell and Co²⁺ is reduced in the Co/Zr cell

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