$A$ reaction,$Ni_{(s)} + Cu^{2+}_{(aq)} \rightarrow Ni^{2+}_{(aq)} + Cu_{(s)}$ occurs in a cell. Calculate $E^0_{cell}$ if $E^0_{Cu} = 0.337 \ V$ and $E^0_{Ni} = -0.257 \ V$. (in $V$)

Given,for $Sn^{4+} / Sn^{2+}$,standard reduction potential is $0.15 \ V$ and for $Au^{3+} / Au$,standard reduction potential is $1.5 \ V$. For the reaction,$3 Sn^{2+} + 2 Au^{3+} \longrightarrow 3 Sn^{4+} + 2 Au$,the value of $E_{\text{cell}}^{\circ}$ is:

For a Galvanic cell consisting of a zinc electrode and a standard hydrogen electrode,$E^{\circ}(Zn^{+2}_{(aq)} \mid Zn_{(s)}) = -0.76 \ V$. Identify the reaction that takes place at the positive electrode during the working of the cell.

Electrode potentials $(E^o)$ are given below:
$Cu^{+}/Cu = +0.52 \ V$
$Fe^{3+}/Fe^{2+} = +0.77 \ V$
$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$
$Ag^{+}/Ag = +0.88 \ V$
Based on the above potentials,the strongest oxidizing agent will be:

The standard electrode potential $(E^\circ)$ for the reaction $Zn^{2+}_{(aq)} + 2e^- \rightarrow Zn_{(s)}$ is $-0.76 \ V$. What is the standard electrode potential for the reaction $2Zn_{(s)} \rightarrow 2Zn^{2+}_{(aq)} + 4e^-$?

If standard reduction potentials $(E^0)$ of $(Al^{+3}(aq)|Al(s))$, $(Fe^{+2}(aq)|Fe(s))$, $(Cu^{+2}(aq)|Cu(s))$ and $(Ag^{+1}(aq)|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?