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 of silver in grams per coulomb (g-C^(-1)), we can follow these steps:

### Step 1: Understand the definition of electrochemical equivalent (E)
The electrochemical equivalent (E) of an element is defined as the mass of the element that is deposited or liberated during electrolysis when one coulomb of electric charge is passed through the electrolyte. It can be expressed mathematically as:

\[ E = \frac{M}{nF} \]

Where:
- \( E \) = electrochemical equivalent (g-C^(-1))
- \( M \) = molar mass of the element (g/mol)
- \( n \) = number of moles of electrons transferred per mole of the element
- \( F \) = Faraday's constant (approximately 96500 C/mol)

### Step 2: Identify the molar mass of silver (Ag)
The molar mass of silver (Ag) is given as 108 g/mol.

### Step 3: Determine the number of electrons transferred (n)
For silver, which typically forms a +1 ion (Ag^+), one mole of silver corresponds to the transfer of one mole of electrons. Therefore, \( n = 1 \).

### Step 4: Use Faraday's constant (F)
The value of Faraday's constant \( F \) is approximately 96500 C/mol.

### Step 5: Substitute the values into the formula
Now we can substitute the values into the formula for electrochemical equivalent:

\[ E = \frac{M}{nF} = \frac{108 \text{ g/mol}}{1 \times 96500 \text{ C/mol}} \]

### Step 6: Calculate the electrochemical equivalent
Now, performing the calculation:

\[ E = \frac{108}{96500} \approx 0.00112 \text{ g-C}^{-1} \]

### Final Answer
The electrochemical equivalent of silver is approximately **0.00112 g-C^(-1)**.

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