For the cell reaction: \( 4 \mathrm{Br}^{-}+\mathrm{O}_{2}+4 \mathrm{H}^{+} \rightleftharpoons 2....

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Question For the cell reaction: \( 4 \mathrm{Br}^{-}+\mathrm{O}_{2}+4 \mathrm{H}^{+} \rightleftharpoons 2 \mathrm{Br}_{2}+2 \mathrm{H}_{2} \mathrm{O} \); \( \mathrm{E}^{\circ}=0.18 \mathrm{~V} \). The value of \( \left(\log \mathrm{K}_{\mathrm{C}}\right) \) at \( 298 \mathrm{~K} \) is \( [2.303 \) \( \mathrm{RT} / \mathrm{F}=0.06] \)
(A) 12
(B) 6
(C) 18
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