If 10 faradays of electricity are passed through sodium chloride solution, how many moles of chlorine gas are formed?

When determining the amount of chlorine gas formed from the electrolysis of sodium chloride (NaCl) solution, it is important to consider the chemical reactions occurring at the anode and cathode.

In the electrolysis of sodium chloride solution, chlorine gas is produced at the anode. The relevant half-reaction for chlorine gas formation is:

[ 2Cl^- \rightarrow Cl_2 + 2e^- ]

This indicates that two moles of chloride ions (Cl⁻) are required to produce one mole of chlorine gas (Cl₂).

Now, we need to relate the amount of charge (expressed in faradays) to the moles of chlorine produced. One faraday corresponds to the charge required to produce one mole of monovalent ions (like Cl⁻) at an electrode, which is 96485 coulombs. Since the reaction produces one mole of Cl₂ from two moles of Cl⁻, passing 2 faradays yields 1 mole of Cl₂.

Given that 10 faradays are passed through the solution, we can calculate the moles of chlorine produced using the stoichiometric relationship derived from the half-reaction. Since it takes 2 faradays to produce 1 mole of