If the standard reduction potential `E^(@)` for four divalent elements X,Y,Z, W are `-1.46V, -0.36V, 0.15V and -1.24V` respectively then

Options

A. X will replace `Z^(2+)` from aqueous solution
B. Y will replace `Z^(2+)` from aqueous solution
C. W will replace `Z^(2+)` from aqueous solution
D. All statements are correct

Answer

To solve the problem, we need to analyze the standard reduction potentials of the given divalent elements (X, Y, Z, and W) and determine which of them can replace the \( Z^{2+} \) ion in an aqueous solution.

### Step-by-Step Solution:

1. **Identify the Standard Reduction Potentials**:
- For element X: \( E^\circ = -1.46 \, V \)
- For element Y: \( E^\circ = -0.36 \, V \)
- For element Z: \( E^\circ = 0.15 \, V \)
- For element W: \( E^\circ = -1.24 \, V \)

2. **Understanding Replacement Reaction**:
- A metal can replace another metal ion in solution if it has a higher reduction potential. This means that the metal being replaced (in this case, Z) must have a lower reduction potential than the metal trying to replace it.

3. **Compare Reduction Potentials**:
- **For X to replace Z**:
- \( E^\circ(Z) = 0.15 \, V \) (Z)
- \( E^\circ(X) = -1.46 \, V \) (X)
- Since \( 0.15 \, V > -1.46 \, V \), X can replace Z.

- **For Y to replace Z**:
- \( E^\circ(Y) = -0.36 \, V \) (Y)
- Again, \( 0.15 \, V > -0.36 \, V \), so Y can also replace Z.

- **For W to replace Z**:
- \( E^\circ(W) = -1.24 \, V \) (W)
- Here, \( 0.15 \, V > -1.24 \, V \), indicating that W can replace Z as well.

4. **Conclusion**:
- Since all three elements (X, Y, and W) have lower reduction potentials than Z, they can all replace \( Z^{2+} \) in an aqueous solution.

5. **Final Answer**:
- The correct option is D: All statements are correct.