If $Cu^{+} + e^- \to Cu$ ; $E^o = X_1$ and $Cu^{2+} + 2e^- \to Cu$ ; $E^o = X_2$,then the value of $E^o$ for $Cu^{2+} + e^- \to Cu^{+}$ will be:

In a cell reaction
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$
$E_{cell}^o = + 0.46 \ V$.
If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be

$A$ 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 $V$)

At $25^\circ C$,$1 \, atm$ of gas $X$ is bubbled through a solution containing $1 \, M$ $Y^-$ and $1 \, M$ $Z^-$. If the reduction potential order is $Z > Y > X$,then:

What is to be done to determine the potential of any half cell?

The standard electrode potentials of $Ag^{+}/Ag$,$Hg_2^{2+}/2Hg$,$Cu^{2+}/Cu$,and $Mg^{2+}/Mg$ are $0.80 \ V$,$0.79 \ V$,$0.34 \ V$,and $-2.37 \ V$,respectively. An aqueous solution containing $1 \ M$ concentration of each of these metal salts is electrolyzed. With increasing voltage,what is the correct sequence of deposition of the metals at the cathode?