If the electrode potential of $Zn^{2+} | Zn$ is $-0.76 \, V$ and the potential of $Cu^{2+} | Cu$ is $0.34 \, V$,what will be the $EMF$ of the cell formed by both electrodes in $V$?

What is the $e.m.f.$ of the cell in $V$?
$Cr | Cr^{3+} (1.0 \ M) || Co^{2+} (1.0 \ M) | Co$
Given: $E^{o}$ for $Cr^{3+} | Cr = -0.74 \ V$ and $Co^{2+} | Co = -0.28 \ V$

Bubbles of gas $z$ are evolved from a solution containing $x$ and $y$. If the order of reduction potential is $x > y > z$,then:

If the emf of the cell $Cu(s) | Cu^{2+}(1M) || Ag^+(1M) | Ag(s)$ is $0.463 \text{ V}$ at $25^{\circ} \text{C}$ and the standard electrode potential of the $Cu$ electrode is $0.337 \text{ V}$, find the standard electrode potential of the $Ag$ electrode. (in $\text{ V}$)

Given $:$
$(i) \, Cu^{2+} + 2e^- \rightarrow Cu \,, \, E^o = 0.337 \, V$
$(ii) \, Cu^{2+} + e^- \rightarrow Cu^{+} \,, \, E^o = 0.153 \, V$
Electrode potential,$E^o$ for the reaction,
$Cu^{+} + e^- \rightarrow Cu \,,$ will be $............$ $V$.

Calculate the $E_{cell}^o$ for $Zn_{(s)}|Zn_{(1M)}^{2+}| |Cd_{(1M)}^{2+}|Cd_{(s)}$ at $25^{\circ} C$ given that $E_{Zn^{2+}/Zn}^{\circ} = -0.763 \ V$ and $E_{Cd^{2+}/Cd}^{\circ} = -0.403 \ V$. (in $V$)