Which one of the following reactions does not | vedclass

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(D) The reaction $Br_2 + 2Cl^- \longrightarrow 2Br^- + Cl_2$ does not take place because the standard cell potential $E^{\circ}_{cell}$ is negative,ma

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$Br_2 + 2Cl^- \longrightarrow 2Br^- + Cl_2$

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(D) The reaction $Br_2 + 2Cl^- \longrightarrow 2Br^- + Cl_2$ does not take place because the standard cell potential $E^{\circ}_{cell}$ is negative,making the reaction non-spontaneous. For this reaction: Cathode: $Br_2 + 2e^- \longrightarrow 2Br^-$; $E^{\circ} = 1.09 \ V$ Anode: $2Cl^- \longrightarrow Cl_2 + 2e^-$; $E^{\circ} = 1.36 \ V$ $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode} = 1.09 \ V - 1.36 \ V = -0.27 \ V$. Since $E^{\circ}_{cell} In contrast,$F_2$,$Cl_2$,and $Br_2$ can oxidize the halide ions below them in the group,resulting in positive $E^{\circ}_{cell}$ values for the other options.

Which one of the following reactions does not take place?

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