The standard reduction potential values of three metallic cations of $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ are $0.52, -3.03$ and $-1.18 \mathrm{V}$, respectively. The order of reducing power of the corresponding metals is

A solution is one molar in each of $\mathrm{NaCl}, {\mathrm{CdCl}}_2,$ ${\mathrm{ZnCl}}_2$ and ${\mathrm{PbCl}}_2.$ To this, tin metal is added. Which of the following is true ? Given :-

${{{\mathrm{E}}^{\circ }}_{\mathrm{Pb}}}^{2+}{/}_{\mathrm{Pb}}=-0.126 \mathrm{V}, \mathrm{E}{{°}_{\mathrm{Sn}}}^{{}^{2+}}{/}_{\mathrm{Sn}}=-0.136 \mathrm{V},$

$\mathrm{E}{{°}_{\mathrm{Cd}}}^{2+}{/}_{\mathrm{Cd}}=–0.40 \mathrm{V}, \mathrm{E}{{°}_{\mathrm{Zn}}}^{2+}{/}_{\mathrm{Zn}}=–0.763 \mathrm{V},$

$\mathrm{E}{{°}_{\mathrm{Na}}}^{+}{/}_{\mathrm{Na}}=–2.71 \mathrm{V},$

Electrode potential data are given below

${\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{3+}+{\mathrm{e}}^{-}⟶{\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{2+}; \mathrm{E}°=+0.77 \mathrm{V}$

${\mathrm{Al}}_{\left(\mathrm{aq}\right)}^{3+}+3{\mathrm{e}}^{-}⟶{\mathrm{Al}}_{\left(\mathrm{s}\right)}; \mathrm{E}°=-1.66 \mathrm{V}$

${\mathrm{Br}}_{2\left(\mathrm{aq}\right)}+2{\mathrm{e}}^{-}⟶2{\mathrm{Br}}_{\left(\mathrm{aq}\right)}^{-}; \mathrm{E}°=+1.66 \mathrm{V}$

Based on the above data which statement(s) is incorrect?

${\mathrm{Ag}}_2\mathrm{O}+{\mathrm{H}}_2\mathrm{O}+2{\mathrm{e}}^{-}⟶2\mathrm{Ag}+2{\mathrm{OH}}^{-}$

In the above chemical reaction