The reaction frac{1}{2} H_{2(g)} + AgCl_{(s)} | vedclass

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(C) In the given reaction: $1$. $H_{2(g)}$ is oxidized to $H^+_{(aq)}$ at the anode: $\frac{1}{2} H_{2(g)} \rightarrow H^+_{(aq)} + e^-$. $2$. $AgCl_{

Vedclass · Accepted Answer

$Pt | H_{2(g)} | HCl_{(aq)} || AgCl_{(s)} | Ag$

Vedclass · Answer

(C) In the given reaction: $1$. $H_{2(g)}$ is oxidized to $H^+_{(aq)}$ at the anode: $\frac{1}{2} H_{2(g)} \rightarrow H^+_{(aq)} + e^-$. $2$. $AgCl_{(s)}$ is reduced to $Ag_{(s)}$ at the cathode: $AgCl_{(s)} + e^- \rightarrow Ag_{(s)} + Cl^-_{(aq)}$. $3$. The cell representation is $Pt | H_{2(g)} | H^+_{(aq)}, Cl^-_{(aq)} | AgCl_{(s)} | Ag$. $4$. This corresponds to the cell $Pt | H_{2(g)} | HCl_{(aq)} || AgCl_{(s)} | Ag$.

The reaction $\frac{1}{2} H_{2(g)} + AgCl_{(s)} \rightarrow H^+_{(aq)} + Cl^-_{(aq)} + Ag_{(s)}$ occurs in which of the following galvanic cells?

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