The electrochemical equivalent for zinc `(` atomic weight `=65.4)` is `……………………………` .

Explanation

To find the electrochemical equivalent (Z) for zinc, we can use the formula:

\[ Z = \frac{M}{n \cdot F} \]

where:
- \( M \) is the molar mass (atomic weight) of the element,
- \( n \) is the number of moles of electrons transferred per mole of the substance,
- \( F \) is Faraday's constant, approximately \( 96500 \, \text{C/mol} \).

### Step-by-Step Solution:

1. **Identify the Molar Mass (M) of Zinc:**
The atomic weight of zinc is given as \( 65.4 \, \text{g/mol} \).
\[ M = 65.4 \, \text{g/mol} \]

2. **Determine the Number of Electrons Transferred (n):**
Zinc typically undergoes a reduction reaction where it gains 2 electrons to form zinc metal (Zn).
\[ n = 2 \]

3. **Use Faraday's Constant (F):**
The value of Faraday's constant is approximately \( 96500 \, \text{C/mol} \).
\[ F = 96500 \, \text{C/mol} \]

4. **Substitute Values into the Formula:**
Now, substitute the values of \( M \), \( n \), and \( F \) into the formula for electrochemical equivalent.
\[ Z = \frac{65.4}{2 \times 96500} \]

5. **Calculate the Electrochemical Equivalent (Z):**
First, calculate the denominator:
\[ 2 \times 96500 = 193000 \]
Now, perform the division:
\[ Z = \frac{65.4}{193000} \approx 3.38 \times 10^{-4} \, \text{g/C} \]

### Final Answer:
The electrochemical equivalent for zinc is:
\[ Z \approx 3.38 \times 10^{-4} \, \text{g/C} \]

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