Products of Electrolysis Summary

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Products of Electrolysis Summary

Electrolysis is a chemical process that uses electric current to drive a non-spontaneous chemical reaction. The products of electrolysis depend on the substances involved and the type of electrolyte used. Here are some common examples:

  1. Electrolysis of Water (H₂O):
    • Cathode (Reduction): 2H2O+2e−→H2(g)+2OH−2H_2O + 2e^- \rightarrow H_2(g) + 2OH^-2H2​O+2e−→H2​(g)+2OH−
    • Anode (Oxidation): 2H2O→O2(g)+4H++4e−2H_2O \rightarrow O_2(g) + 4H^+ + 4e^-2H2​O→O2​(g)+4H++4e−
    • Overall Reaction: 2H2O→2H2(g)+O2(g)2H_2O \rightarrow 2H_2(g) + O_2(g)2H2​O→2H2​(g)+O2​(g)
    • Products: Hydrogen gas (H₂) and oxygen gas (O₂)
  2. Electrolysis of Sodium Chloride Solution (Brine):
    • Cathode (Reduction): 2H2O+2e−→H2(g)+2OH−2H_2O + 2e^- \rightarrow H_2(g) + 2OH^-2H2​O+2e−→H2​(g)+2OH−
    • Anode (Oxidation): 2Cl−→Cl2(g)+2e−2Cl^- \rightarrow Cl_2(g) + 2e^-2Cl−→Cl2​(g)+2e−
    • Overall Reaction: 2NaCl+2H2O→2NaOH+H2(g)+Cl2(g)2NaCl + 2H_2O \rightarrow 2NaOH + H_2(g) + Cl_2(g)2NaCl+2H2​O→2NaOH+H2​(g)+Cl2​(g)
    • Products: Hydrogen gas (H₂), chlorine gas (Cl₂), and sodium hydroxide (NaOH)
  3. Electrolysis of Molten Sodium Chloride:
    • Cathode (Reduction): Na++e−→Na(l)Na^+ + e^- \rightarrow Na(l)Na++e−→Na(l)
    • Anode (Oxidation): 2Cl−→Cl2(g)+2e−2Cl^- \rightarrow Cl_2(g) + 2e^-2Cl−→Cl2​(g)+2e−
    • Overall Reaction: 2NaCl(l)→2Na(l)+Cl2(g)2NaCl(l) \rightarrow 2Na(l) + Cl_2(g)2NaCl(l)→2Na(l)+Cl2​(g)
    • Products: Sodium metal (Na) and chlorine gas (Cl₂)
  4. Electrolysis of Copper Sulfate Solution:
    • Cathode (Reduction): Cu2++2e−→Cu(s)Cu^{2+} + 2e^- \rightarrow Cu(s)Cu2++2e−→Cu(s)
    • Anode (Oxidation with inert anode like platinum): 2H2O→O2(g)+4H++4e−2H_2O \rightarrow O_2(g) + 4H^+ + 4e^-2H2​O→O2​(g)+4H++4e−
    • Overall Reaction (with inert anode): 2CuSO4+2H2O→2Cu(s)+O2(g)+2H2SO42CuSO_4 + 2H_2O \rightarrow 2Cu(s) + O_2(g) + 2H_2SO_42CuSO4​+2H2​O→2Cu(s)+O2​(g)+2H2​SO4​
    • Products (with inert anode): Copper metal (Cu), oxygen gas (O₂), and sulfuric acid (H₂SO₄)

In cases where a copper anode is used:

  • Anode (Oxidation with copper anode): Cu(s)→Cu2++2e−Cu(s) \rightarrow Cu^{2+} + 2e^-Cu(s)→Cu2++2e−
  • Overall Reaction (with copper anode): CuSO4→Cu(s)+CuSO4CuSO_4 \rightarrow Cu(s) + CuSO_4CuSO4​→Cu(s)+CuSO4​
  • Products (with copper anode): Copper metal (Cu) (no net reaction since copper is dissolved and deposited)

The exact products of electrolysis depend on the materials and conditions used in the process, such as the type of electrolyte, the nature of the electrodes (inert or reactive), and the applied voltage.

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