Given the electrode potential of Copper to be +0.34V and that if Zinc should be −0.76V, calculate the emf of…

Question

Given the electrode potential of Copper to be +0.34V and that if Zinc should be −0.76V, calculate the emf of the cell

ScanSolve AI Tutor · Accepted Answer

To calculate the electromotive force (emf) of the cell, we use the standard electrode potentials of copper and zinc.

Identify the standard electrode potentials.
The standard electrode potential for copper, $E^{\circ}_{\text{Cu}}$ , is $+0.34\,\text{V}$ .
The standard electrode potential for zinc, $E^{\circ}_{\text{Zn}}$ , is $-0.76\,\text{V}$ .
Determine the cathode and anode.
The species with the more positive (or less negative) standard electrode potential will be reduced and act as the cathode. Copper has a more positive potential ( $+0.34\,\text{V}$ ) than zinc ( $-0.76\,\text{V}$ ). Therefore, copper will be reduced at the cathode, and zinc will be oxidized at the anode.
Apply the formula for cell emf.
The emf of the cell is calculated using the formula:
$E_{\text{cell}} = E^{\circ}_{\text{cathode}} - E^{\circ}_{\text{anode}}$
Substitute the values and calculate.
$E_{\text{cell}} = (+0.34\,\text{V}) - (-0.76\,\text{V})$ $E_{\text{cell}} = 0.34\,\text{V} + 0.76\,\text{V}$ $E_{\text{cell}} = 1.10\,\text{V}$
The emf of the cell is $\text{+1.10 V}$ .

Given the electrode potential of Copper to be +0.34V and that if Zinc should be -0.76V, calculate the emf of the cell