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

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Question

(B) The given cell reaction is: $\frac{1}{2} H_{2(g)} + AgCl_{(s)} \rightleftharpoons H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$.At the anode,oxidation

Vedclass · Accepted Answer

$Pt \mid H_{2(g)} \mid HCl_{(aq)} \mid AgCl_{(s)} \mid Ag_{(s)}$

Vedclass · Answer

(B) The given cell reaction is: $\frac{1}{2} H_{2(g)} + AgCl_{(s)} \rightleftharpoons H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$.At the anode,oxidation occurs: $\frac{1}{2} H_{2(g)} \rightarrow H^{+}_{(aq)} + e^-$.At the cathode,reduction occurs: $AgCl_{(s)} + e^- \rightarrow Ag_{(s)} + Cl^{-}_{(aq)}$.Combining these,we get the overall reaction. This corresponds to a cell with a hydrogen electrode $(Pt \mid H_2)$ and a silver-silver chloride electrode $(AgCl \mid Ag)$ in an $HCl$ solution.Therefore,the correct cell representation is $Pt \mid H_{2(g)} \mid HCl_{(aq)} \mid AgCl_{(s)} \mid Ag_{(s)}$.

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

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Using the above information,find the ion which will be deposited first at the cathode if a solution containing $A^{2+}_{(aq.)}$ and $B^{3+}_{(aq.)}$ is electrolysed.

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