Question:
A constant current of 30 A is passed through an aqueous solution of NaCl for a time of 1.00 h. What is the volume of Cl\(_2\) gas at STP produced?
A constant current of 30 A is passed through an aqueous solution of NaCl for a time of 1.00 h. What is the volume of Cl\(_2\) gas at STP produced?
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Faraday's law can be used to relate the amount of substance produced in an electrolysis reaction to the current and time.
Updated On: Jan 6, 2026
- 30.0L
- 25.0L
- 12.5L
- 11.2L
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The Correct Option is A
Solution and Explanation
Step 1: Calculating moles of Cl\(_2\) produced.
Using Faraday's law and the molar volume of gas at STP, the volume of \( \text{Cl}_2 \) gas produced can be calculated by considering the number of moles of electrons involved.
Step 2: Conclusion.
The volume of Cl\(_2\) gas produced is 30.0L, corresponding to option (1).
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