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In the cell Pt(s)|H(2)(g,1bar)|HCl (aq)|...

In the cell `Pt(s)|H_(2)(g,1bar)|HCl (aq)| AgCl(s)|Ag(S)|Pt(s)` the cell potential is 0.92V when a `10^(-6)` mola1 HCl Ssolution is used. The standard electrode potential of `(ACl//Ag,Cl^(-))` electrode is :
`{given, (2.30Rt)/(F) = 0.6V at 298K}`

A

`(0.40V)`

B

`(0.76V)`

C

`0.20V`

D

`0.94V`

Text Solution

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To solve the problem step by step, we will analyze the electrochemical cell and apply the Nernst equation to find the standard electrode potential of the AgCl/Ag electrode. ### Step 1: Identify the half-cell reactions In the given electrochemical cell: - At the anode (oxidation half-reaction): \[ \text{H}_2(g) \rightarrow 2\text{H}^+(aq) + 2e^- \] ...
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