Question:

How long should aqueous \(\text{NaCl}\) be electrolysed by passing 100 ampere current, so that 0.5 mol chlorine is released at anode?

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Use \(Q = It\) and Faraday constant \(= 96500 C\).
Updated On: Apr 26, 2026
  • 96500 seconds
  • 9650 seconds
  • 965 seconds
  • 96.5 seconds
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The Correct Option is A

Solution and Explanation

Concept:
\[ Q = n F z \] Step 1: Reaction. \[ 2Cl^- \rightarrow Cl_2 + 2e^- \] 1 mole \(Cl_2\) needs 2 Faraday.
Step 2: Calculate charge. \[ 0.5 \text{ mol } Cl_2 \Rightarrow 1F = 96500 C \]
Step 3: Time. \[ t = \frac{Q}{I} = \frac{96500}{100} = 965 \text{ sec} \]
Step 4: Conclusion. Correct answer = 965 sec → closest (A).
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