The cell $\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left(1\mathrm{M}\right)\Vert {\mathrm{Cu}}^{2+}\left(1\mathrm{M}\right)\right|\mathrm{Cu}:\left({\mathrm{E}}_{\mathrm{coll}}°=1.10\mathrm{V}\right)$ was allowed to completely discharge at $298\mathrm{K}$ The relative concentration of ${\mathrm{Zn}}^{2+}$ to ${\mathrm{Cu}}^{2+}\left(\frac{\left[{\mathrm{Zn}}^{2+}\right]}{\left[{\mathrm{Cu}}^{2+}\right]}\right)$ is: (Take $\frac{1.1}{0.059}=18.65$).

Given: ${\mathrm{E}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^0=-0.72,{\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^0=-0.42\mathrm{V}$

The potential for the cell $\mathrm{Cr}\left|{\mathrm{Cr}}^{3+}(0.1\mathrm{M})\Vert {\mathrm{Fe}}^{2+}(0.01\mathrm{M})\right|\mathrm{Fe}$ at $298\mathrm{K}$ (Take $\frac{2.303\mathrm{R}\left(298\right)}{\mathrm{F}}=0.06$)

Given: ${\mathrm{E}}_{{\mathrm{F}}_{\mathrm{e}}^{3+}/{\mathrm{F}}_{\mathrm{e}}}^0=-0.036\mathrm{V}, {\mathrm{E}}_{{\mathrm{Fa}}^{2+}/\mathrm{Fe}}^0=-0.439\mathrm{V}$

The value of standard electrode potential for the change, ${\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{3+}+{\mathrm{e}}^{-}⟶{\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{2+}$ will be:

$\frac{2}{3}{\text{Al}}_{\text{2}}{\text{O}}_{\text{3}}\to \frac{4}{3}\text{Al}+{\text{O}}_{\text{2}}, \mathrm{\Delta }\text{G}=+966 {\text{kJ mol}}^{\text{-1}}$

The reduction potential of hydrogen half-cell will be negative if:

The standard reduction potential for ${\mathrm{Zn}}^{\mathrm{2+}}/\mathrm{Zn}, {\mathrm{Ni}}^{\mathrm{2+}}/\mathrm{Ni} \text{and} {\mathrm{Fe}}^{\mathrm{2+}}/\mathrm{Fe}$ are $-0.76 \mathrm{V}, -0.23 \mathrm{V} \mathrm{and} -0.44 \mathrm{V}$, respectively. The reaction $\mathrm{X}+{\mathrm{Y}}^{+2}\stackrel{}{\to } {\mathrm{X}}^{2+}+\mathrm{Y}$ will be spontaneous when ______.

Given: ${\mathrm{E}}_{{\mathrm{Cr}}^{3+}/\mathrm{cr}}^0=-0.74\mathrm{V}; {\mathrm{E}}_{{\mathrm{MnO}}_4^{-}/{\mathrm{Mn}}^{2+}}^0=1.51\mathrm{V}$

${\mathrm{E}}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+}}=1.33\mathrm{V};{\mathrm{E}}_{\mathrm{Cl}/{\mathrm{Cl}}^{-}}^0=1.36\mathrm{V}$

Based on the data given above, the strongest oxidising agent will be: