In the electrolysis of `CuCl_(2)` solution (aq) with Cu electrodes, the weight of cathode increased by 3.2 g. In the anode,

Options

A. 0.05 mole of `Cu^(2+)` will go into the solution
B. 560 of `O_(2)` will be liberated
C. 112 mL of `Cl_(2)` will be liberated
D. 3.2 mole of `Cu^(2+)` will go into the solution

Answer

To solve the problem regarding the electrolysis of a copper(II) chloride (CuCl₂) solution using copper electrodes, we need to analyze the changes occurring at both the cathode and anode during the process.

### Step-by-Step Solution:

1. **Understanding the Electrolysis Process**:
- During electrolysis, the solution of CuCl₂ dissociates into Cu²⁺ ions and Cl⁻ ions. The copper ions (Cu²⁺) migrate towards the cathode (negative electrode), while chloride ions (Cl⁻) migrate towards the anode (positive electrode).

2. **Cathode Reaction**:
- At the cathode, Cu²⁺ ions gain electrons (reduction) and are deposited as metallic copper:
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu (s)} \]
- Given that the weight of the cathode increased by 3.2 g, this weight corresponds to the amount of copper deposited.

3. **Calculating Moles of Copper Deposited**:
- The molar mass of copper (Cu) is approximately 63.5 g/mol. To find the number of moles of copper deposited, we use the formula:
\[ \text{Moles of Cu} = \frac{\text{Weight of Cu}}{\text{Molar Mass of Cu}} = \frac{3.2 \, \text{g}}{63.5 \, \text{g/mol}} \approx 0.0504 \, \text{mol} \]

4. **Anode Reaction**:
- At the anode, copper metal from the anode is oxidized to Cu²⁺ ions:
\[ \text{Cu (s)} \rightarrow \text{Cu}^{2+} + 2e^- \]
- For every mole of copper that is oxidized, one mole of Cu²⁺ ions is produced.

5. **Weight Loss at the Anode**:
- Since the same amount of copper that is deposited at the cathode is oxidized at the anode, the weight loss at the anode will be equal to the weight gain at the cathode, which is 3.2 g.

### Conclusion:
- The weight of the anode decreases by 3.2 g as copper is oxidized to Cu²⁺ ions during the electrolysis process.