The chemical reaction,2AgCl_{(s)} + H_{2(g)} | vedclass

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Question

(C) The given cell reaction is $2AgCl_{(s)} + H_{2(g)} 	o 2HCl_{(aq)} + 2Ag_{(s)}$.In this reaction,$H_2$ is oxidized to $H^+$ at the anode,and $AgCl

Vedclass · Accepted Answer

$Pt_{(s)} | H_{2(g)}, 1 \ bar | 1 \ M \ HCl_{(aq)} | AgCl_{(s)} | Ag_{(s)}$

Vedclass · Answer

(C) The given cell reaction is $2AgCl_{(s)} + H_{2(g)} 	o 2HCl_{(aq)} + 2Ag_{(s)}$.In this reaction,$H_2$ is oxidized to $H^+$ at the anode,and $AgCl$ is reduced to $Ag$ at the cathode.The anode is a standard hydrogen electrode represented as $Pt_{(s)} | H_{2(g)}, 1 \ bar | H^+_{(aq)}$.The cathode involves the $Ag/AgCl$ electrode,represented as $Cl^-_{(aq)} | AgCl_{(s)} | Ag_{(s)}$.Combining these,the cell notation is $Pt_{(s)} | H_{2(g)}, 1 \ bar | 1 \ M \ HCl_{(aq)} | AgCl_{(s)} | Ag_{(s)}$.

The chemical reaction,$2AgCl_{(s)} + H_{2(g)} \to 2HCl_{(aq)} + 2Ag_{(s)}$ taking place in a galvanic cell is represented by the notation:

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