Question

Number of coulombs corresponding to \(1\) mol of electrons approximately is equal to

• A. \(1.93\times 10^5\)
• B. \(9.65\times 10^4\)
• C. \(1.93\times 10^4\)
• D. \(9.65\times 10^5\)

Hint:

One Faraday is the charge of one mole of electrons and is approximately \(96500\,C\).

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
This question asks for the value of the Faraday constant (F). The Faraday constant represents the magnitude of electric charge per mole of electrons. It is the product of two fundamental constants: the elementary charge (charge of a single electron) and Avogadro's number (the number of particles in one mole).
Step 2: Key Formula or Approach:
The Faraday constant (F) is calculated as: \[ F = N_A \times e \] where: - $N_A$ is Avogadro's number, approximately $6.022 \times 10^{23}$ mol$^{-1}$. - $e$ is the elementary charge, approximately $1.602 \times 10^{-19}$ Coulombs.
Step 3: Detailed Explanation:
We need to calculate the total charge of 1 mole of electrons. \[ \text{Total Charge} = (\text{Number of electrons in one mole}) \times (\text{Charge of one electron}) \] \[ F = (6.022 \times 10^{23}) \times (1.602 \times 10^{-19}) \text{ C/mol} \] \[ F \approx 9.647 \times 10^4 \text{ C/mol} \] This value is commonly approximated for calculations as 96500 C/mol, or $9.65 \times 10^4$ C/mol. Step 4: Final Answer:
The charge corresponding to 1 mole of electrons is approximately $9.65 \times 10^4$ Coulombs. This is the Faraday constant. Therefore, option (B) is correct.