Which of the following reactions will be spon | vedclass

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(B) For a reaction to be spontaneous in an electrochemical cell,the cell potential $E_{cell}^0$ must be positive.$E_{cell}^0 = E_{cathode}^0 - E_{anod

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

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(B) For a reaction to be spontaneous in an electrochemical cell,the cell potential $E_{cell}^0$ must be positive.$E_{cell}^0 = E_{cathode}^0 - E_{anode}^0$.Given $E_{Cl_2 \mid 2Cl^-}^0 = 1.36 \ V$ and $E_{Br_2 \mid 2Br^-}^0 = 1.09 \ V$.For option $B$: $2Br^- + Cl_2 \rightarrow Br_2 + 2Cl^-$.Here,$Cl_2$ is reduced to $Cl^-$ (cathode) and $Br^-$ is oxidized to $Br_2$ (anode).$E_{cell}^0 = E_{Cl_2 \mid 2Cl^-}^0 - E_{Br_2 \mid 2Br^-}^0 = 1.36 \ V - 1.09 \ V = 0.27 \ V$.Since $E_{cell}^0 > 0$,the reaction is spontaneous.

Which of the following reactions will be spontaneous in an electrochemical cell constructed from the given standard electrode potentials: $E_{Cl_2 \mid 2Cl^-}^0 = 1.36 \ V$ and $E_{Br_2 \mid 2Br^-}^0 = 1.09 \ V$?

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