Copper metal, $\mathrm{Cu}\left(\mathrm{s}\right)$, is oxidised to ${\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$, while ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ is reduced to silver metal, $\mathrm{Ag}\left(\mathrm{s}\right)$, then the equilibrium greatly lies in favour of

Which is the best description of behaviour of bromine in the given equation?

${\mathrm{H}}_2\mathrm{O}+{\mathrm{Br}}_2⟶\mathrm{HBr}+\mathrm{HOBr}$

For the galvanic cell in which the following reaction takes place, $\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+2}\left(\mathrm{aq}\right)⟶{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$ write individual reaction at each electrode.

Calculate ${\mathrm{E}}^{\mathrm{o}}$ for the cell: $\mathrm{AI}\left|{\mathrm{Al}}^{3+}\right(1\mathrm{M}\left)\right|\left|{\mathrm{Cu}}^{2+}\right(1\mathrm{M}\left)\right|\mathrm{Cu}$

Given, ${\mathrm{E}}_{{\mathrm{Al}}^{3+}/\mathrm{Al}}^0$ and ${\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^0$ are $-1.66 \mathrm{V}$ and $+0.34 \mathrm{V}$ respectively.

Balance the following equation

${\mathrm{Br}}_2+{\mathrm{H}}_2{\mathrm{O}}_2⟶{\mathrm{BrO}}_3+{\mathrm{H}}_2\mathrm{O}$ (in acidic medium)