For the following cell,the standard electrode | vedclass

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(C) The standard cell potential $E_{cell}^0$ is calculated using the formula: $E_{cell}^0 = E_{cathode}^0 - E_{anode}^0$.In the given cell $Zn | Zn^{2

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$1.10$

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(C) The standard cell potential $E_{cell}^0$ is calculated using the formula: $E_{cell}^0 = E_{cathode}^0 - E_{anode}^0$.In the given cell $Zn | Zn^{2+} || Cu^{2+} | Cu$,$Zn$ acts as the anode and $Cu$ acts as the cathode.Given: $E_{Cu^{2+}/Cu}^0 = 0.34 \ V$ and $E_{Zn^{2+}/Zn}^0 = -0.76 \ V$.Substituting the values: $E_{cell}^0 = 0.34 \ V - (-0.76 \ V) = 0.34 \ V + 0.76 \ V = 1.10 \ V$.

For the following cell,the standard electrode potential $E_{cell}^0$ is . . . . . . .
$E_{Zn^{2+}/Zn}^0 = -0.76 \ V, E_{Cu^{2+}/Cu}^0 = 0.34 \ V$
$Zn | Zn^{2+} || Cu^{2+} | Cu$ (in $V$)

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For the following cell,the standard electrode potential $E_{cell}^0$ is . . . . . . .$E_{Zn^{2+}/Zn}^0 = -0.76 \ V, E_{Cu^{2+}/Cu}^0 = 0.34 \ V$$Zn | Zn^{2+} || Cu^{2+} | Cu$ (in $V$)