What is the electrochemical equivalent (in g-`C^(-1)` ) of silver?

Options

A. 108 F
B. `108//F`
C. `F//108`
D. `1//108 F`

Answer

To find the electrochemical equivalent (Z) of silver, we can follow these steps:

### Step 1: Understand the Formula for Electrochemical Equivalent
The electrochemical equivalent (Z) is given by the formula:
\[ Z = \frac{E}{F} \]
where:
- \( E \) is the equivalent weight of the substance (in grams),
- \( F \) is Faraday's constant, approximately \( 96500 \, C \, mol^{-1} \).

### Step 2: Calculate the Equivalent Weight of Silver
The equivalent weight (E) can be calculated using the formula:
\[ E = \frac{M}{n} \]
where:
- \( M \) is the molar mass of silver,
- \( n \) is the number of moles of electrons transferred per mole of silver in the reaction.

For silver (Ag):
- The molar mass (M) of silver is approximately \( 108 \, g/mol \).
- The valency (or n factor) of silver in its common ionic form (Ag\(^+\)) is \( 1 \).

Thus, we can calculate the equivalent weight:
\[ E = \frac{108 \, g/mol}{1} = 108 \, g \]

### Step 3: Substitute the Values into the Electrochemical Equivalent Formula
Now we can substitute the values into the electrochemical equivalent formula:
\[ Z = \frac{E}{F} = \frac{108 \, g}{96500 \, C} \]

### Step 4: Calculate the Electrochemical Equivalent
Now, perform the calculation:
\[ Z = \frac{108}{96500} \, g/C \]

### Step 5: Simplify the Result
Calculating the above expression gives:
\[ Z \approx 0.00112 \, g/C \]

### Final Answer
Thus, the electrochemical equivalent of silver is approximately:
\[ Z \approx 0.00112 \, g/C \]

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