Faraday constant is defined as

Options

A. Charge carried by 1 electron
B. Charge carried by one mole of electrons
C. Charge required to deposit one mole of substance
D. Charge carried by two moles of electrons

Explanation

**Step-by-Step Solution:**

1. **Understanding Faraday Constant:**
The Faraday constant (F) is defined as the amount of electric charge carried by one mole of electrons. It is a fundamental constant in electrochemistry.

2. **Value of Faraday Constant:**
The value of the Faraday constant is approximately 96500 coulombs per mole (C/mol). This means that one mole of electrons carries a charge of about 96500 coulombs.

3. **Charge of a Single Electron:**
The charge of a single electron is approximately \(1.6 \times 10^{-19}\) coulombs (C).

4. **Calculating Charge for One Mole of Electrons:**
To find the total charge carried by one mole of electrons, we multiply the charge of a single electron by Avogadro's number (\(6.022 \times 10^{23}\) mol\(^{-1}\)):
\[ \text{Charge for one mole of electrons} = \text{Charge of one electron} \times \text{Avogadro's number} \]
\[ = (1.6 \times 10^{-19} \, \text{C}) \times (6.022 \times 10^{23} \, \text{mol}^{-1}) \]

5. **Performing the Calculation:**
\[ = 1.6 \times 6.022 \times 10^{4} \, \text{C} \]
\[ = 9.6352 \times 10^{4} \, \text{C} \approx 96500 \, \text{C} \]

6. **Conclusion:**
Therefore, the Faraday constant is defined as the charge carried by one mole of electrons, which is approximately 96500 coulombs.