---
title: "In an industrial process, molten sodium chloride, \\(\\text{NaCl}(l)\\), is electrolyzed in an electrochemical cell according to the following overall reaction:  \\[ 2\\,\\text{NaCl}(l) \\rightarrow 2\\,\\text{Na}(l) + \\text{Cl}_2(g) \\]  A constant electric current of \\(9.65\\text{ A}\\) is passed through the molten salt for \\(100.0\\text{ minutes}\\). Given that Faraday’s constant is \\(96{,}500\\text{ C/mol } e^-\\), what is the total number of moles of electrons transferred through the cell during this process?"
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url: "https://nerd-notes.com/ubq/120015/"
date_modified: "2026-08-21T08:31:54+00:00"
---

# In an industrial process, molten sodium chloride, \(\text{NaCl}(l)\), is electrolyzed in an electrochemical cell according to the following overall reaction:

\[ 2\,\text{NaCl}(l) \rightarrow 2\,\text{Na}(l) + \text{Cl}_2(g) \]

A constant electric current of \(9.65\text{ A}\) is passed through the molten salt for \(100.0\text{ minutes}\). Given that Faraday’s constant is \(96{,}500\text{ C/mol } e^-\), what is the total number of moles of electrons transferred through the cell during this process?

In an industrial process, molten sodium chloride, \(\text{NaCl}(l)\), is electrolyzed in an electrochemical cell according to the following overall reaction:

\[ 2\,\text{NaCl}(l) \rightarrow 2\,\text{Na}(l) + \text{Cl}_2(g) \]

A constant electric current of \(9.65\text{ A}\) is passed through the molten salt for \(100.0\text{ minutes}\). Given that Faraday's constant is \(96{,}500\text{ C/mol } e^-\), what is the total number of moles of electrons transferred through the cell during this process?

- **A.** \(0.00500\text{ mol}\)
- **B.** \(0.0100\text{ mol}\)
- **C.** \(0.300\text{ mol}\)
- **D.** \(0.600\text{ mol}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120015/*