Why is molten sodium chloride rather than solid sodium chloride used as the electrolyte?

Solid-state does not allow the movement of ions and unsuitable for electrolysis. When melted at high temperature, sodium chloride separates into sodium and chloride ions, so that, electrolysis can take place to form sodium atom and chlorine gas.

What is the difference between aqueous sodium chloride and molten sodium chloride?

In molten sodium chloride, the only available ions are Na+ and Cl−. With electrolysis, the products will be sodium metal and chlorine gas. In an aqueous solution, the sodium chloride still moves the charges from one electrode to the other, but the potential for electrolysis of water is less than Na+ or Cl−.

Can aqueous NaCl solution be used for the extraction of sodium?

An aqueous solution of sodium chloride is not used for electrolytic reduction of sodium metal because if we electrolyse an aqueous solution of sodium chloride, then as soon as sodium metal is produced at the cathode, it will react with water to form sodium hydroxide.

Why is molten salt used in electrolysis?

Deduce the products of the electrolysis of a molten salt: Electrolysis of a molten salt produces the elements from the salt. So, the electrolysis of WCl4 produces W and Cl2. Metal ions receive electrons at the negative electrode, and the non-metals lose them at the positive electrode.

How does the product of the electrolysis of molten sodium chloride differ from that of brine?

It may be logical to assume that the electrolysis of aqueous sodium chloride, called brine, would yield the same result through the same reactions as the process in molten NaCl. However, the reduction reaction that occurs at the cathode does not produce sodium metal, instead, the water is reduced.

What is the difference between a molten and aqueous solution?

The key difference between molten and aqueous is that the term molten refers to the liquid state of materials liquified by heat, whereas the term aqueous refers to the liquid state of materials that are liquified by dissolving in water.

What is the difference between molten and aqueous?

Why in electrolysis molten liquid is used instead of solid?

The reason that an electrolyte has to be molten or in solution is that the current is carried through the electrolyte by the movement of ions – not electrons. In a solid, those ions can’t move.

How is sodium obtained from molten sodium chloride?

Textbook solution The extraction of metal from its molten state is done by the process of Electrolysis. If we melt Sodium Chloride above 801° C then the two electrodes will be inserted namely Cathode and Anode into the melt. Sodium ions migrate to the cathode where electrons enter the melt and we get sodium metal.

What is the difference between molten NaCl and aqueous NaCl?

The products obtained from the electrolysis of molten NaCl and aqueous NaCl are different. Explain? In the electrolysis of molten NaCl, sodium is deposited at the cathode while chlorine gas is liberated at anode.

What is the product of electrolysis of molten sodium chloride?

Electrolysis is done with an iron cathode and graphite anode and iron gauze preventing the mixing of products chlorine and sodium. The products of molten sodium chloride are sodium metal and chlorine gas. Electrolysis of Aqueous Sodium Chloride Sodium chloride is dissociated and exists as sodium and chloride ions in aqueous solution.

What is the difference between electrolysis of NaCl and aqueous solution?

Expert Answer: In the electrolysis of molten NaCl, sodium is deposited at the cathode while chlorine gas is liberated at anode. Where as in the electrolysis of aqueous solution of NaCl, Cl 2 gas is liberated at anode and H 2 gas is liberated at cathode. Answered by | 4th Jun, 2014, 03:23: PM

What happens when sodium chloride is melted at high temperature?

When melted at high temperature, sodium chloride separates into sodium and chloride ions, so that, electrolysis can take place to form sodium atom and chlorine gas. Read More In Detail: Electrolysis NaCl → Na + (l) + Cl – (l) At cathode: reduction of 2Na + (l) + e – → Na (l)