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. 30.0L
• B. 25.0L
• C. 12.5L
• D. 11.2L

Hint:

Faraday's law can be used to relate the amount of substance produced in an electrolysis reaction to the current and time.

Answer 1

The Correct Option is A

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).