Statement 1: The standard emf `(E_(cell)^(@))` of following concentration cell is zero.
`Zn(s)|ZnSO_(4)(C_(1))||ZnSO_(4)(C_(2))|Zn(s)`
Statement 2: The electrolyte concentration cell will be is greater in cathodic half-cell.

Options

A. Statement 1 is true, statement 2 is true, statement 2 is a correct explanation for statement 1
B. Statement 1 is true, statement 2 is true, statement 2 is not a correct explanation for statement 1
C. Statement 1 is true, statement 2 is false
D. statement 1 is false,statement 2 is true

Explanation

To analyze the statements provided in the question, we will break down the concepts involved in the concentration cell and the electrochemical principles that govern it.

### Step-by-Step Solution:

1. **Understanding the Concentration Cell**:
- The given concentration cell is represented as:
\[ \text{Zn(s)} | \text{ZnSO}_4(C_1) || \text{ZnSO}_4(C_2) | \text{Zn(s)} \]
- In this cell, both half-cells contain the same metal (Zn) and the same type of electrolyte (ZnSO4) but at different concentrations (C1 and C2).

2. **Standard EMF of the Cell**:
- The standard EMF (E°) of a concentration cell is calculated using the formula:
\[ E°_{\text{cell}} = E°_{\text{cathode}} - E°_{\text{anode}} \]
- Since both half-cells involve the same metal, the standard electrode potentials (E°) for both the cathode and anode are equal, leading to:
\[ E°_{\text{cell}} = 0 \]
- Therefore, **Statement 1** is correct: The standard EMF of the concentration cell is zero.

3. **Understanding the Cathodic and Anodic Reactions**:
- In a concentration cell, the half-cell with the higher concentration (C2) acts as the cathode, while the half-cell with the lower concentration (C1) acts as the anode.
- The cell reaction can be described as:
\[ \text{Zn}^{2+}(C_2) + 2e^- \rightarrow \text{Zn(s)} \quad (\text{cathode}) \]
\[ \text{Zn(s)} \rightarrow \text{Zn}^{2+}(C_1) + 2e^- \quad (\text{anode}) \]

4. **Evaluating Statement 2**:
- Statement 2 claims that the electrolyte concentration in the cathodic half-cell will be greater than that in the anodic half-cell.
- This is true, as the cathodic half-cell (C2) has a higher concentration than the anodic half-cell (C1).
- Thus, **Statement 2** is also correct.

5. **Conclusion**:
- Both statements are true, but Statement 2 does not explain why the standard EMF is zero. It merely states a fact about the concentrations in the half-cells without linking it to the EMF being zero.

### Final Answer:
- **Statement 1** is true: The standard EMF \( E°_{\text{cell}} \) of the concentration cell is zero.
- **Statement 2** is true: The electrolyte concentration in the cathodic half-cell is greater than that in the anodic half-cell.
- However, Statement 2 does not provide a valid explanation for Statement 1.