Answer the following: Explain electrolysis of molten NaCl. - Chemistry

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Answer in Brief

Answer the following:

Explain electrolysis of molten NaCl.

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Solution

  1. Construction of cell:
    The electrolytic cell consists of a container in which fused NaCl is placed. Two graphite electrodes are immersed in it. They are connected by metallic wires to a source of direct current that is the battery. The carbon electrode connected to the terminal electrode of the battery is an anode and that connected to the negative terminal of the battery is the cathode.
  2. Reactions occurring in the cell:
    Fused NaCl contains Na+ and Cl ions which are freely mobile. When potential is applied, the cathode attracts Na+ ions and anode attracts Cl ions. As these are charged particles, their migration results in an electric current. When these ions reach the respective electrodes, they are discharged according to the following reactions.
    1. Oxidation half-reaction at anode:
      1. Cl ions migrate to anode. Each Cl ion, that reaches anode, gives one electron to anode. It oxidizes to neutral Cl atom in the primary process. Two Cl atoms then combine to form chlorine gas in the secondary process.
      2. `2"Cl"_(("l"))^(-) -> "Cl"_(("g")) +
        "Cl"_(("g")) + 2"e"^(-)`      (primary process)
        `"Cl"_(("g")) + "Cl"_(("g")) -> "Cl"_(2("g"))`
        (secondary process)
        `2"Cl"_(("l"))^(-) -> "Cl"_(2("g")) + 2"e"^(-)`  (overall oxidation)
      3. The battery sucks electrons so produced at the anode and pushes them to cathode through a wire in an external circuit. Thus, the battery serves as an electron pump. The electrons from the battery enter into solution through cathode and leave the solution through anode.
    2. Reduction half reaction at cathode:
      1. The electrons supplied by the battery are used in cathodic reduction. Each Na+ ion, that reaches cathode accepts an electron from the cathode and reduces to metallic sodium.
      2. `"Na"_(("l"))^+ + "e"^(-) -> "Na"_(("l"))`
    3. Net cell reaction:
      1. The net cell reaction is the sum of two electrode reactions.
      2. `2"Cl"_(("l"))^(-) -> "Cl"_(2("g")) + 2"e"^(-)`    (Oxidation half reaction)
      3. `2"Na"_(("l"))^+ + 2"e"^(-) -> 2"Na"_(("l"))`  (Reduction half reaction)
      4. `2"Na"_(("l"))^+ + 2"Cl"_(("l"))^(-) -> 2"Na"_(("l")) + "Cl"_(2("g"))`   (Overall cell reaction)
  3. Results of electrolysis of molten NaCl:
    i) A pale green Cl2 gas is released at anode.
    ii) Molten silvery-white sodium is formed at the cathode.
    iii) The decomposition of NaCl into metallic sodium and Cl2(g) is nonspontaneous. The electrical energy supplied by the battery forces the reaction to occur.
Concept: Electrolytic Cell
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Chapter 5: Electrochemistry - Exercises [Page 118]

APPEARS IN

Balbharati Chemistry 12th Standard HSC for Maharashtra State Board
Chapter 5 Electrochemistry
Exercises | Q 4.02 | Page 118

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