For the cell reaction,$A_{(s)} + B^{2+}_{(aq)} \rightarrow A^{2+}_{(aq)} + B_{(s)}$,if the equilibrium constant of the reaction is $10^4$ at $298 \ K$,what is the standard $EMF$ of the cell (in $V$)?

If $E^{\circ}(Mg^{+2}_{(aq)} \mid Mg_{(s)}) = -2.37 \ V$. What is the potential for $Mg_{(s)} \rightarrow Mg^{+2}_{(0.01 \ M)} + 2 \overline{e}$ at $298 \ K$?

The electrode potential of a chlorine electrode is maximum when the concentration of chloride ion in the solution (in $mol \ L^{-1}$) is $X$. What is the value of $X$?

For a certain redox reaction in a galvanic cell $X(s) + Y^{2+}_{(aq)} \rightarrow X^{2+}_{(aq)} + Y(s)$, $E^0_{cell}$ is $0.0296 \text{ V}$ at $298 \text{ K}$. What is the equilibrium constant of the reaction?

For a certain redox reaction in a galvanic cell $X(s) + Y^{2+}(aq) \rightarrow X^{2+}(aq) + Y(s)$, $E^0_{cell} = 0.0296 \text{ V}$ at $298 \text{ K}$. What is the equilibrium constant $(K_c)$ of the reaction?

$1 \ F$ electricity was passed through $Cu^{2+} (1.5 \ M, 1 \ L) / Cu$ and $0.1 \ F$ was passed through $Ag^{+} (0.2 \ M, 1 \ L) / Ag$ electrolytic cells. After this,the two cells were connected to make an electrochemical cell. The $emf$ of the cell thus formed at $298 \ K$ is:
Given: $E^0_{Cu^{2+} / Cu} = 0.34 \ V$,$E^0_{Ag^{+} / Ag} = 0.8 \ V$,$\frac{2.303 \ RT}{F} = 0.06 \ V$ (in $V$)