Given the standard electrode potentials,
${\mathrm{K}}^{+}/\mathrm{K} =-2.93 \mathrm{V} ,$
${\mathrm{Ag}}^{+}/\mathrm{Ag}=0.80 \mathrm{V} ,$
${\mathrm{Hg}}^{2+}/\mathrm{Hg}=0.79 \mathrm{V} ,$
${\mathrm{Mg}}^{2+}/\mathrm{Mg}=-2.37 \mathrm{V} ,$
${\mathrm{Cr}}^{3+}/\mathrm{Cr}=-0.74 \mathrm{V}$
Arrange these metals in their increasing order of reducing power.

Depict the galvanic cell in which the reaction $\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$ takes place. Further show:

(i) which of the electrode is negatively charged,

(ii) the carriers of the current in the cell, and

(iii) individual reaction at each electrode