The reaction 1/2 H_{2(g)} + AgCl_{(s)} to H^{ | vedclass

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(C) The given cell reaction is: $1/2 H_{2(g)} + AgCl_{(s)} 	o H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$.In this reaction,$H_2$ is oxidized to $H^+$ at

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

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(C) The given cell reaction is: $1/2 H_{2(g)} + AgCl_{(s)} 	o H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$.In this reaction,$H_2$ is oxidized to $H^+$ at the anode,and $AgCl$ is reduced to $Ag$ at the cathode.The anode reaction is: $1/2 H_{2(g)} 	o H^{+}_{(aq)} + e^{-}$,which corresponds to a standard hydrogen electrode $(Pt | H_{2(g)}, HCl_{(soln)})$.The cathode reaction is: $AgCl_{(s)} + e^{-} 	o Ag_{(s)} + Cl^{-}_{(aq)}$,which corresponds to a silver-silver chloride electrode $(AgCl_{(s)} | Ag)$.Therefore,the cell representation is $Pt | H_{2(g)}, HCl_{(soln)} || AgCl_{(s)} | Ag$.

The reaction $1/2 H_{2(g)} + AgCl_{(s)} \to H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$ occurs in the galvanic cell:

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