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.(c) When the electrode wires are switched in one of the cells, which cell will run as the voltaic cell and which as the electrolytic cell?

Answer 1

Au/Cr cell will run as a voltaic cell and Co/Zn cell will run as an electrolytic cell.

What is an electrolytic cell?

An electrolytic cell that uses electrical energy to enable a non-spontaneous redox reaction is known as an electrolytic cell.

Certain chemicals can be electrolyzed using electrolytic cells, which are electrochemical cells.

For example, water can be electrolyzed to create gaseous oxygen and gaseous hydrogen with the use of an electrolytic cell.

The following are the three essential parts of electrolytic cells:

Cathode (which is negatively charged for electrolytic cells)

Anode (which is positively charged for electrolytic cells)

Electrolyte

The reactions for each half cell is given by

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

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

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

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

When the Au/Cr cell will run as a voltaic cell and Co/Zn cell will run as an electrolytic cell, the a difference in the voltages is produced

$E^o_{series} = E^o_{Au/Cr} - E^o_{Co/Zn}$  = 2.24 V – 0.48 V = 1.76 V

Learn more about electrolytic cell:

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