A current of `2.68 A` is passed for `1.0` hour through an aqueous solution of `CuSO_(4)` using copper electrodes.
Which of the following statements is `//` are correct ?

Options

A. Increase in mass of cathode = 3.175 g
B. Decrease in mass of anode = 3.175 g
C. No change in mass of electrodes
D. The ratio between the change in mass of cathode to anode is 1 : 2

Explanation

To solve the problem, we need to analyze the electrolysis of copper sulfate (CuSO₄) using copper electrodes and determine the changes in mass at the cathode and anode.

### Step-by-Step Solution:

1. **Determine the total charge passed:**
- Current (I) = 2.68 A
- Time (t) = 1 hour = 3600 seconds
- Total charge (Q) can be calculated using the formula:
\[ Q = I \times t = 2.68 \, \text{A} \times 3600 \, \text{s} = 9648 \, \text{C} \]

2. **Calculate the number of Faradays:**
- The number of Faradays (F) can be calculated using the formula:
\[ F = \frac{Q}{96500} = \frac{9648}{96500} \approx 0.1 \, \text{Faraday} \]

3. **Identify the reactions at the electrodes:**
- At the cathode (reduction):
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu (s)} \]
- At the anode (oxidation):
\[ \text{Cu (s)} \rightarrow \text{Cu}^{2+} + 2e^- \]

4. **Calculate the mass of copper deposited at the cathode:**
- From Faraday's laws, 2 Faradays deposit 1 mole of copper (Cu).
- Therefore, 0.1 Faraday will deposit:
\[ \text{Moles of Cu} = \frac{0.1}{2} = 0.05 \, \text{moles} \]
- Mass of copper deposited:
\[ \text{Mass} = \text{moles} \times \text{molar mass} = 0.05 \, \text{moles} \times 63.5 \, \text{g/mol} = 3.175 \, \text{g} \]

5. **Calculate the mass of copper dissolved at the anode:**
- The same amount of copper that is deposited at the cathode will dissolve at the anode.
- Therefore, the mass of copper dissolved at the anode is also:
\[ 3.175 \, \text{g} \]

6. **Conclusion:**
- The mass of copper deposited at the cathode is 3.175 g.
- The mass of copper dissolved at the anode is also 3.175 g.
- Hence, the increase in mass at the cathode is equal to the decrease in mass at the anode.

### Correct Statements:
1. The mass of copper deposited at the cathode is 3.175 g (Correct).
2. The mass of copper dissolved at the anode is 3.175 g (Correct).
3. There is a change in mass of the electrodes (Incorrect).

### Summary:
- The correct statements are:
- The mass of copper deposited at the cathode is 3.175 g.
- The mass of copper dissolved at the anode is 3.175 g.