The equilibrium constant for the following general reaction is $10^{30}$. Calculate $E^o$ for the cell at $298 \ K$.
$2 X_2(s)+3 Y^{2+}(a q) \rightarrow 2 X_2^{3+}(a q)+3 Y(s)$

Calculate $\Delta G$ and $E_{cell}$ for the following cell at $298 \ K$ temperature.
$Al_{(s)} | Al^{3+} (0.01 \ M) || Fe^{2+} (0.02 \ M) | Fe_{(s)}$ $\left[ E^o_{Al^{3+}|Al} = -1.66 \ V \right.$ and $\left. E^o_{Fe^{2+}|Fe} = -0.44 \ V \right]$

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

Calculate the electrode potential at $298 \; K$ for $Zn|Zn^{2+}$ electrode in which the activity of zinc ions is $0.001 \; M$ and $E^o_{Zn^{2+}/Zn}$ is $-0.76 \; V$. (in $; V$)

In a cell,a copper electrode was used as a cathode. What is the electrode potential (in $V$) of the copper electrode dipped in $0.1 \ M \ Cu^{2+}$ solution at $298 \ K$?
$(E_{Cu^{2+}/Cu}^{\ominus} = 0.34 \ V; \frac{2.303 \ RT}{F} = 0.06 \ V)$

Which of the following statements is correct regarding the $emf$ of the cell for the cell reaction,$Cd_{(s)} + Cu^{2+}_{(aq)} \longrightarrow Cd^{2+}_{(aq)} + Cu_{(s)}$,if the concentration of $Cd^{2+}$ is $10$ times greater than the concentration of $Cu^{2+}_{(aq)}$ at $298 \ K$?