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(A) In a cell representation, the anode (oxidation) is written on the left and the cathode (reduction) on the right.$1$. Oxidation half-reaction: $Mg_

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$Mg_{(s)} \mid Mg^{2+}_{(aq)} \parallel Cl_{2(g)} \mid Cl^{-}_{(aq)} \mid Pt_{(s)}$

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(A) In a cell representation, the anode (oxidation) is written on the left and the cathode (reduction) on the right.$1$. Oxidation half-reaction: $Mg_{(s)} \rightarrow Mg^{2+}_{(aq)} + 2e^-$. This occurs at the anode: $Mg_{(s)} \mid Mg^{2+}_{(aq)}$.$2$. Reduction half-reaction: $Cl_{2(g)} + 2e^- \rightarrow 2Cl^-_{(aq)}$. This occurs at the cathode. Since $Cl_2$ is a gas, an inert electrode like $Pt$ is used: $Cl_{2(g)} \mid Cl^-_{(aq)} \mid Pt_{(s)}$.$3$. Combining these with the salt bridge $(\parallel)$, the representation is $Mg_{(s)} \mid Mg^{2+}_{(aq)} \parallel Cl_{2(g)} \mid Cl^-_{(aq)} \mid Pt_{(s)}$.

Which is the correct symbolic representation for the following cell reaction?
$Mg_{(s)} + Cl_{2(g)} \rightarrow Mg^{2+}_{(aq)} + 2Cl^{-}_{(aq)}$

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Which is the correct symbolic representation for the following cell reaction?$Mg_{(s)} + Cl_{2(g)} \rightarrow Mg^{2+}_{(aq)} + 2Cl^{-}_{(aq)}$