Question

On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for E^Θ value).

$$\mathrm{Br}{\phantom{A}}_2+2\mathrm{Cl}{\phantom{A}}^{-}⟶\mathrm{Cl}{\phantom{A}}_2+2\mathrm{Br}{\phantom{A}}^{-}$$

Answer 1

Here $$\mathrm{Br}$$ undergoes reduction thus acting as cathode and $$\mathrm{Cl}$$ acting as the anode.

For cathode E^Θcathode = 1.09 V

For anode E^Θanode = 1.36 V

E^Θcell = – 0.25

The negative potential prevents easy reaction, so the redox reaction will not occur.