When electrolysis of silver nitrate solution is carried out using silver electrodes, wich of the following reaction occurs at the anode?

Options

A. `Ag toAg^(+)+e^(-)`
B. `Ag^(+)+e^(-)toAg`
C. `2H_(2)Oto4H^(+)+O_(2)+4e^(-)`
D. `4OH^(-)to2H_(2)+O_(2)+4e^(-)`

Answer

To determine the reaction that occurs at the anode during the electrolysis of silver nitrate solution using silver electrodes, we can follow these steps:

### Step 1: Understand the Electrolysis Process
Electrolysis involves the breakdown of a compound in solution by passing an electric current through it. In this case, we are dealing with silver nitrate (AgNO₃) solution.

### Step 2: Identify the Components in the Solution
When silver nitrate is dissolved in water, it dissociates into silver ions (Ag⁺) and nitrate ions (NO₃⁻). Therefore, the solution contains Ag⁺ and NO₃⁻ ions.

### Step 3: Determine the Anode Reaction
At the anode, oxidation occurs. This means that a substance loses electrons. Since we are using silver electrodes, silver (Ag) will undergo oxidation.

### Step 4: Write the Oxidation Reaction
The oxidation reaction at the anode can be represented as:
\[ \text{Ag (s)} \rightarrow \text{Ag}^+ (aq) + e^- \]

This equation shows that solid silver (Ag) loses one electron (e⁻) to become silver ions (Ag⁺).

### Step 5: Conclusion
Thus, the reaction that occurs at the anode during the electrolysis of silver nitrate solution using silver electrodes is:
\[ \text{Ag (s)} \rightarrow \text{Ag}^+ (aq) + e^- \]