Question

In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under STP condition. The current to be passed is

• A. 1.93 A
• B. 9.65 A
• C. 19.3 A
• D. 0.965 A

Hint:

At STP, 1 mole of gas occupies 22,400 cc. Use $I = \frac{\text{equivalents} \times F}{t}$ for electrolysis.

Answer 1

The Correct Option is B

Step 1: Determine Moles of $H_2$
Number of moles of $H_2 = \frac{Volume}{Molar~Volume} = \frac{1.12}{22400}$.
Step 2: Determine Equivalents
Number of equivalents of hydrogen $= \frac{1.12 \times 2}{22400} = 10^{-4}$.
Step 3: Apply Faraday's Law
Number of Faradays required $= 10^{-4}$. Current $I = \frac{Q}{t} = \frac{nF}{t}$.
Step 4: Calculation
Current to be passed in one second $= 96500 \times 10^{-4} = 9.65$ A.
Final Answer: (b)