For the cell reaction with the indicated concentrations
$Al_{(s)} + 3Ag^{+}_{(aq)} \, (0.10 \, M) \to Al^{3+}_{(aq)} \, (0.30 \, M) + 3Ag_{(s)}$,
the measured voltage $(E_{cell})$ is $1.50 \, V$. Calculate $E^o_{cell} \, ........... \, V$
Given: $\frac{2.303 \, RT}{F} = 0.06 \, V ; \, \log \, 3 = 0.48$

$A$ hydrogen electrode is made by dipping platinum wire in a solution of nitric acid of $pH=9$ and passing hydrogen gas around the platinum wire at $1.2 \ atm$ pressure. The oxidation potential of such an electrode equals $V$.

In a cell reaction,a $2$ electron change occurs. The standard $e.m.f.$ of the cell at $25^\circ C$ is $0.295 \ V$. What is the equilibrium constant for the reaction at $25^\circ C$?

For the cell $Co | Co^{+2} (C_2) || Co^{+2} (C_1) | Co$,$\Delta G$ is negative if

At $25\,^{\circ}C$,calculate the equilibrium constant for the cell reaction,
$X_{(s)} + Y_{(aq)}^{2+} \rightleftharpoons Y_{(s)} + X_{(aq)}^{2+}$
Given:
$E_{X^{2+}/X}^{o} = -1.36\,V$;
$E_{Y^{2+}/Y}^{o} = -0.76\,V$; $\frac{2.303\,RT}{F} = 0.06$

One half cell in a voltaic cell is constructed by dipping a silver rod in an $AgNO_3$ solution of unknown concentration, and the other half cell is a $Zn$ rod dipped in a $1 \text{ M}$ solution of $ZnSO_4$. $A$ voltage of $1.60 \text{ V}$ is measured at $298 \text{ K}$ for this cell. What is the concentration of $Ag^+$ ions in terms of $\log x$ (where $x = [Ag^+]$)? Given: $E^\ominus_{Zn^{2+}/Zn} = -0.76 \text{ V}$, $E^\ominus_{Ag^+/Ag} = +0.80 \text{ V}$, and $\frac{2.303RT}{F} = 0.059 \text{ V}$.