Question

What is the number of faraday required to form 1 mol \( \text{H}_2 \) by reduction of \( \text{H}^+ \) ions?

• A. 4
• B. 2
• C. 0.5
• D. 1

Hint:

Check the stoichiometry of electrons in the balanced half-reaction.

Answer 1

The Correct Option is B

Step 1: Concept
The number of Faradays required is equal to the number of moles of electrons transferred in the redox reaction.

Step 2: Meaning
Faraday's law relates the chemical change to the quantity of electricity.

Step 3: Analysis
The reduction half-reaction is: \(2H^+ + 2e^- \rightarrow H_{2(g)}\).

Step 4: Conclusion
To produce 1 mole of \(H_2\), 2 moles of electrons are required, which corresponds to 2 Faradays. Final Answer: (B)