Which of the following reactions is correct f | vedclass

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(A) In an electrochemical cell representation,the left side represents the anode (oxidation) and the right side represents the cathode (reduction).Ano

Vedclass · Accepted Answer

$2Br_{(aq)}^{-} + Cl_{2(g)} \rightarrow Br_{2(g)} + 2Cl_{(aq)}^{-}$

Vedclass · Answer

(A) In an electrochemical cell representation,the left side represents the anode (oxidation) and the right side represents the cathode (reduction).Anode reaction (oxidation): $2Br_{(aq)}^{-} \rightarrow Br_{2(g)} + 2e^{-}$Cathode reaction (reduction): $Cl_{2(g)} + 2e^{-} \rightarrow 2Cl_{(aq)}^{-}$Adding these two half-reactions gives the overall cell reaction:$2Br_{(aq)}^{-} + Cl_{2(g)} \rightarrow Br_{2(g)} + 2Cl_{(aq)}^{-}$Therefore,the correct option is $A$.

Which of the following reactions is correct for a given electrochemical cell at $25^{\circ} C$ ?
$Pt | Br_{2(g)} | Br_{(aq)}^{-} || Cl_{(aq)}^{-} | Cl_{2(g)} | Pt$

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Which of the following reactions is correct for a given electrochemical cell at $25^{\circ} C$ ?$Pt | Br_{2(g)} | Br_{(aq)}^{-} || Cl_{(aq)}^{-} | Cl_{2(g)} | Pt$