Using E deg(Cl2/Cl-) = 1.36 V, E deg(Br2/Br-) = 1.09 V and F = 96500 C mol^-1, the standard Gibbs energy change for Cl2 + 2Br- -> 2Cl- + Br2 is

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Using $E^{\circ} (Cl X_{2} / Cl X^{-}) = 1.36 V$ , $E^{\circ} (Br X_{2} / Br X^{-}) = 1.09 V$ and $F = 96500 C mo l^{- 1}$ , the standard Gibbs energy change for $Cl X_{2} + 2 Br X^{-} 2 Cl X^{-} + Br X_{2}$ is

E_{ce ll}^{\circ} = 1.36 - 1.09 = 0.27 V

with

n = 2

electrons.

Δ G^{\circ} = - n F E^{\circ} = - 2 (96500) (0.27) = - 52110 J = - 52.1 kJ mo l^{- 1}

. The value is negative, so chlorine displaces bromine.