Which statement is incorrect about cell constant

Options

A. Cell constant depends on the distance between the electrodes and their area of cross section
B. The dimension of cell constant is `"length"^(-1)`
C. The cell constant `G^(**)=Rk`
D. none of the above

Answer

To determine which statement is incorrect about the cell constant, we will analyze the definition and properties of the cell constant step by step.

### Step-by-Step Solution:

1. **Understanding Cell Constant**:
- The cell constant (K) is defined as the ratio of the distance between the electrodes (L) to the area of the cross-section of the electrodes (A).
- Mathematically, it is expressed as:
\[ K = \frac{L}{A} \]

2. **Components of the Cell Constant**:
- Here, L is the distance between the electrodes (measured in centimeters or meters).
- A is the area of the cross-section of the electrodes (measured in square centimeters or square meters).
- Therefore, the unit of the cell constant is inverse length (e.g., cm⁻¹ or m⁻¹).

3. **Analyzing Statements**:
- **Statement 1**: "The cell constant depends on the distance between the electrodes and their area."
- This statement is correct because the cell constant is directly defined by L and A.

- **Statement 2**: "The dimension of the cell constant is length inverse."
- This statement is also correct, as we derived that the unit of the cell constant is indeed inverse length (cm⁻¹ or m⁻¹).

- **Statement 3**: "The cell constant is equal to conductance multiplied by conductivity."
- This statement is incorrect. The correct relationship is:
\[ K = R \cdot \sigma \]
where R is resistance and σ is conductivity. The cell constant is not equal to conductance multiplied by conductivity.

4. **Conclusion**:
- Based on the analysis, the incorrect statement about the cell constant is the one that claims it is equal to conductance multiplied by conductivity.

### Final Answer:
The incorrect statement about the cell constant is: "The cell constant is equal to conductance multiplied by conductivity."

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