The voltaic cells are called galvanic cells that produce electrical energy from chemical energy. The cell potential for the cell containing chromium and cobalt is 0.352 V.
The difference between the reduction potentials of the half-cells in an electrochemical cell is defined by the cell potential. It is generated due to the movement of the electrons.
From the galvanic cell, the concentration is given as,
Chromium = 0.01 M
Cobalt = 0.00001 M
The reaction is shown as,
[tex]\rm 2Cr + 3Co^{+2} \rightarrow 2Cr^{+3} + 3Co, n = 6[/tex]
The cell potential is calculated as,
[tex]\begin{aligned} \rm E_{cell} &= \rm E^{\circ}_{cell} - \rm \dfrac {0.059} {n } - log \dfrac{[Cr^{+3}]^{2}}{[Co^{+3}]^{3}}\\\\&= -0.28 - (-0.74) - \dfrac{0.059}{2} - \rm log \dfrac{(0.01)^{2}}{(0.00001)^{3}}\\\\&= 0.352 \rm V \end{aligned}[/tex]
Therefore, 0.352 V is the cell potential for the following voltaic cell.
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