Based on the given data,which is the strongest oxidizing agent? $E_{Li^+|Li}^o = -3.03 \ V$,$E_{Ba^{2+}|Ba}^o = -2.73 \ V$,$E_{Na^+|Na}^o = -2.71 \ V$,and $E_{Mg^{2+}|Mg}^o = -2.37 \ V$.

Give the symbolic representation of the following half-cells (electrodes):
$(i)$ $Zn_{(s)} | Zn^{2+}_{(aq)} (1M)$
$(ii)$ $Cu^{2+}_{(aq)} (1M) | Cu_{(s)}$
$(iii)$ $Pt_{(s)} | H_{2(g)} (1 \text{ bar}) | H^+_{(aq)} (1M)$

Consider the following cell:
$Zn_{(s)} \mid Zn^{2+}_{(1M)} \parallel KCl_{(sat)} \mid Hg_2Cl_{2(paste)} \mid Hg$
$E^{\circ}_{cell} = 1.007 \ V$ and $E^{\circ}_{calomel} = 0.242 \ V$
What is the standard potential of $Zn$ (in $V$)?

The cell reaction of a cell is $Mg_{(s)} + Cu^{2+}_{(aq)} \to Cu_{(s)} + Mg^{2+}_{(aq)}$. If the standard reduction potentials of $Mg$ and $Cu$ are $-2.37 \ V$ and $+0.34 \ V$ respectively,the $EMF$ of the cell is ................. $V$.

Given at $298 \ K$: $E^\ominus_{Fe^{2+}/Fe} = X \ V$; $E^\ominus_{Fe^{3+}/Fe} = Y \ V$. The $E^\ominus_{Fe^{3+}/Fe^{2+}}$ in Volt at $298 \ K$ is given by:

The reaction is spontaneous if the cell potential is