When a solution of `AgNO_3` (1 M) is electrolysed using platinum anode and copper cathode, what are the products obtained at two electrodes?
Given :`E_(cu^(2+)|cu)^(@)=+0.34 "volt", E_(O_2,H^+|H_2O)^(@)=+1.23"volt",E_(H^+|H_2)^(@)=+0.0"volt" E_(ag^+|Ag)^(@)=+0.8 "volt"`

Options

A. `CutoCu^(2+)` at anode, `Ag^+to Ag` at cathode
B. `H_2OtoO_2` at anode, `Cu^(2+)to Cu` at cathode
C. `H_2OtoO_2` at anode, `Ag^+to Ag` at cathode
D. `NO_3^-to NO_2` at anode, `Ag^+to Ag` at cathode

Answer

To solve the problem of identifying the products obtained at the anode and cathode during the electrolysis of a 1 M solution of AgNO₃ using a platinum anode and copper cathode, we will follow these steps:

### Step 1: Identify the half-reactions at the electrodes
In electrolysis, oxidation occurs at the anode and reduction occurs at the cathode. We need to consider the possible half-reactions for both electrodes.

**At the Cathode:**
The possible reduction reactions are:
1. \( \text{Ag}^+ + e^- \rightarrow \text{Ag} \) with \( E^\circ = +0.8 \, \text{V} \)
2. \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \) with \( E^\circ = +0.34 \, \text{V} \)

**At the Anode:**
The possible oxidation reactions are:
1. \( \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \) with \( E^\circ = -0.34 \, \text{V} \) (oxidation potential)
2. \( 2\text{H}_2\text{O} \rightarrow \text{O}_2 + 4H^+ + 4e^- \) with \( E^\circ = -1.23 \, \text{V} \) (oxidation potential)

### Step 2: Determine which reactions are favorable
To determine which reactions will occur, we compare the standard reduction potentials:

- At the cathode, since \( E^\circ \) for Ag is higher than that for Cu, the reduction of Ag⁺ to Ag will occur:
\[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \]

- At the anode, we need to compare the oxidation potentials. The oxidation of Cu has a less negative potential than the oxidation of water, indicating that Cu will oxidize before water:
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \]

### Step 3: Write the overall reactions
From the above analysis, we can summarize the reactions occurring at each electrode:
- **At the Cathode:** Silver is deposited.
\[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \quad (\text{Reduction}) \]

- **At the Anode:** Copper is oxidized to copper ions.
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \quad (\text{Oxidation}) \]

### Conclusion
The products obtained at the electrodes during the electrolysis of a 1 M solution of AgNO₃ are:
- **At the Cathode:** Silver (Ag) is deposited.
- **At the Anode:** Copper ions (Cu²⁺) are produced.

### Final Answer
- **Products at Cathode:** Silver (Ag)
- **Products at Anode:** Copper ions (Cu²⁺)

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