The metals obtained from the molten chloride by the process of electrolytic reduction are

General
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the metals obtained from the molten chloride by the process of electrolytic reduction are

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Which metals are obtained from the molten chloride by the process of electrolytic reduction?

Answer: The metals obtained from molten chloride by the process of electrolytic reduction primarily include alkali metals and alkaline earth metals. This process is a type of electrolysis where molten chloride compounds are decomposed into their elemental components using an electrical current. Let’s explore this process in detail for some specific metals:

Alkali Metals

  1. Sodium (Na):

    • Sodium is typically extracted from molten sodium chloride (NaCl) through the process known as the Downs process.
    • Sodium chloride is mixed with some calcium chloride to lower its melting point.
    • Equation:
      $$\text{2NaCl(l) } \xrightarrow{\text{Electrolysis}}\text{ 2Na(l) + Cl}_2\text{(g)}$$
    • At the cathode, sodium ions are reduced to sodium metal.

  2. Potassium (K):

    • Extraction of potassium can also be conducted from molten potassium chloride (KCl) via electrolysis.
    • Potassium is similar to sodium in behavior and is obtained by reducing potassium ions.

Alkaline Earth Metals

  1. Magnesium (Mg):

    • Magnesium is typically extracted from molten magnesium chloride (MgCl₂).
    • Equation:
      $$\text{MgCl}_2\text{(l) } \xrightarrow{\text{Electrolysis}}\text{ Mg(l) + Cl}_2\text{(g)}$$
    • At the cathode, magnesium ions gain electrons to form magnesium metal.

  2. Calcium (Ca):

    • Calcium can be obtained from the electrolysis of molten calcium chloride (CaCl₂).
    • Similar steps involve the reduction of calcium ions at the cathode.

Process of Electrolytic Reduction

The electrolytic reduction involves:

  • Cathode Reaction: Positive ions (cations) migrate to the cathode, where they gain electrons (reduction) to form the metal.

    • General Reaction: $$\text{M}^{n+} + n\text{e}^- \rightarrow \text{M}$$

  • Anode Reaction: Negative ions (anions) move toward the anode, where they lose electrons (oxidation), often releasing a gaseous byproduct such as chlorine gas (\text{Cl}_2).

    • General Reaction: $$\text{X}^{n-} - n\text{e}^- \rightarrow \text{X}_2$$

Conditions for Electrolytic Reduction

  • High Temperature: Molten state is essential to ensure ions are mobile.
  • Electric Current: An external power source is required to drive the non-spontaneous redox reactions.
  • Inert Electrodes: Often required to prevent reactions with the electrolyte.

Applications

The metals obtained through this process are crucial for various applications:

  • Sodium: Used in street lights, coolant in some nuclear reactors, and as a reducing agent in chemical synthesis.
  • Magnesium: Utilized in the manufacturing of lightweight alloys, in the aerospace industry, and as a reducing agent in the production of pure uranium.

Conclusion

The electrolytic reduction of molten chlorides is a critical industrial process for the extraction of reactive metals such as sodium, potassium, magnesium, and calcium. These metals are pivotal in advancing various technological and industrial fields due to their unique chemical properties.

I hope this helps! If you have any more questions or need further explanation, feel free to ask. @username