When a rod of metal $A$ is dipped in an aqueous solution of metal $B$ (concentration of $B^{2+}$ ion being $1 \ M$) at $25 \ ^oC$,the standard electrode potentials are $E^o_{A^{2+}/A} = -0.76 \ V$ and $E^o_{B^{2+}/B} = +0.34 \ V$. What will happen?

The two half-cell reactions of an electrochemical cell are given as: $Ag^{+} + e^{-} \rightarrow Ag$; $E^{\circ}_{Ag^{+}/Ag} = 0.7995 \ V$ and $Fe^{2+} \rightarrow Fe^{3+} + e^{-}$; $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.7710 \ V$. The value of cell $EMF$ will be: (in $V$)

Using the standard electrode potentials given below,identify the correct statements from the following.
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
$Cu^{2+} + 2e^{-} \longrightarrow Cu ; E^{\circ} = +0.34 \ V$
$Ag^{+} + e^{-} \longrightarrow Ag ; E^{\circ} = +0.80 \ V$
$(i)$ Copper can displace iron from $FeSO_4$ solution.
$(ii)$ Iron can displace copper from $CuSO_4$ solution.
$(iii)$ Silver can displace copper from $CuSO_4$ solution.
$(iv)$ Iron can displace silver from $AgNO_3$ solution.

If more than one species is available near the cathode,which species will undergo a reduction reaction? Provide suitable examples.

What is the observation we get when a gold ring is placed in the solution of $AgNO_3$? $[E_{Ag^{+}|Ag}^o = 0.80 \ V$ and $E_{Au^{3+}|Au}^o = 1.40 \ V]$

$E^{\circ}_{Fe^{2+}/Fe} = -0.441 \ V$ and $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.771 \ V$,the standard $EMF$ of the reaction $Fe + 2Fe^{3+} \rightarrow 3Fe^{2+}$ will be $.......... \ V$.