Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (b) Chlorine gas is evolved as voltage is applied in the cell. Knowing this, identify the electrolyte.

Verified step by step guidance

1. Identify the products of the electrolysis process. Here, chlorine gas (Cl2) is evolved at the anode (carbon electrode).
2. Determine the possible sources of chlorine gas. Chlorine gas is typically produced from chloride ions (Cl-).
3. Consider the common molten salts that contain chloride ions. Magnesium chloride (MgCl2) is a common electrolyte used in the production of magnesium.
4. Analyze the electrolysis reaction. At the anode, chloride ions (Cl-) are oxidized to chlorine gas (Cl2). At the cathode, magnesium ions (Mg2+) are reduced to magnesium metal (Mg).
5. Conclude that the electrolyte used in this electrolysis cell is likely magnesium chloride (MgCl2).

Key Concepts

Electrolysis

Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In this process, an electrolyte is decomposed into its constituent ions when an electric current is passed through it. The electrodes facilitate the movement of ions, leading to the production of substances such as gases or metals at the electrodes.

Electrolyte

An electrolyte is a substance that, when dissolved in a solvent or melted, produces ions that can conduct electricity. In the context of electrolysis, the electrolyte allows the flow of electric current and is essential for the chemical reactions occurring at the electrodes. Common electrolytes include salts, acids, and bases, with molten salts often used in metal extraction processes.

Chlorine Production

Chlorine gas (Cl2) is commonly produced during the electrolysis of sodium chloride (NaCl) solutions or molten NaCl. At the anode, chloride ions (Cl-) are oxidized to form chlorine gas, which is released as a byproduct. Understanding this reaction is crucial for identifying the electrolyte used in the electrolysis cell, as it indicates the presence of chloride ions in the electrolyte.