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The reaction, (1)/(2)H(2)(g) + AgCl(s) H...

The reaction, `(1)/(2)H_(2)(g) + AgCl(s) H^(+)(aq)+Cl^(-) (aq)+Ag(s)`. Occurs in the galvanic cell :

A

`Ag|AgC1((s))|KC1((So1n)|AgNo_(3) | Ag`

B

`PtH_(2)|HC1(So1n)|AgNO_(3) ((so1n)|Ag`

C

`PT|H_(2)((g))|HC1((so1n)| AgC1((S))Ag`

D

`Pt| h_(2)((g))KC1((so1n)|AgC1((S))Ag`

Text Solution

AI Generated Solution

To solve the problem regarding the galvanic cell reaction involving \( \frac{1}{2} H_2(g) + AgCl(s) \rightarrow H^+(aq) + Cl^-(aq) + Ag(s) \), we will follow these steps: ### Step 1: Identify the Oxidation and Reduction Processes In the given reaction, we need to determine which species is being oxidized and which is being reduced. - **Oxidation**: The half-reaction for hydrogen can be written as: \[ \frac{1}{2} H_2(g) \rightarrow H^+(aq) + e^- ...
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