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Grade 10 Chemistry Notes – Chapter 4 Electrochemistry

Chemistry Notes – Grade 10

National Curriculum Pakistan - NCP

Chapter 4: Electrochemistry

Aligned with National Curriculum Pakistan (Federal Board, NBF, PTB)

  1. What are electrochemical cells?
    Electrochemical cells are devices that convert chemical energy into electrical energy or electrical energy into chemical energy.
  2. Name the two types of electrochemical cells.
    Electrolytic cells and galvanic (voltaic) cells.
  3. What is an electrolytic cell?
    An electrochemical cell in which electrical energy is supplied from an external source to drive a non-spontaneous chemical reaction.
  4. What is a galvanic cell?
    A cell that generates electrical energy from a spontaneous redox reaction.
  5. What are electrochemical processes based on?
    They are based on oxidation-reduction (redox) reactions involving the transfer of electrons.
  6. What is a spontaneous reaction?
    A reaction that occurs naturally without external energy input, often releasing energy.
  7. What is a non-spontaneous reaction?
    A reaction that requires continuous energy input to proceed.
  8. Define an electrolyte.
    An electrolyte is a substance that conducts electricity when dissolved in water or molten, due to the presence of free-moving ions.
  9. Give examples of electrolytes.
    Sodium chloride (NaCl), potassium chloride (KCl), hydrochloric acid (HCl), and sodium hydroxide (NaOH).
  10. Define a non-electrolyte.
    A non-electrolyte is a substance that does not conduct electricity in molten or aqueous state because it doesn’t form ions.
  11. Give examples of non-electrolytes.
    Urea, glucose, sucrose, and benzene.
  12. What does an electrolytic cell consist of?
    A vessel with electrolyte solution, two inert electrodes (anode and cathode), and an external power source (battery).
  13. What happens at the anode in an electrolytic cell?
    Oxidation occurs—anions lose electrons.
  14. What happens at the cathode in an electrolytic cell?
    Reduction occurs—cations gain electrons.
  15. Write the general half-reaction at the anode.
    X⁻ → X + e⁻ (oxidation)
  16. Write the general half-reaction at the cathode.
    M⁺ + e⁻ → M (reduction)
  17. What is Down’s Cell used for?
    To extract sodium metal and chlorine gas by electrolysis of molten sodium chloride on an industrial scale.
  18. What are the electrodes in Down’s Cell?
    Iron is used as the cathode and carbon (graphite) as the anode.
  19. Write the anode reaction in Down’s Cell.
    2Cl⁻ → Cl₂(g) + 2e⁻ (oxidation)

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