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अभ्यासक्रम

Electrolysis

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Topics

  • Introduction
  • Experiment

Introduction:

Electrolysis is the process of decomposing a chemical compound into its components using an electric current. It occurs in an electrolytic cell, which consists of: A container with an electrolyte (a liquid or solution containing free ions).

Electrodes:

  • Cathode (negative electrode): Where reduction (gain of electrons) occurs.
  • Anode (positive electrode): Where oxidation (loss of electrons) occurs.

Strong electrolytes like salts, strong acids, and strong bases dissociate completely in water, making them good conductors of electricity and ideal for electrolysis. Pure water, on the other hand, is a poor conductor because it has very few dissociated ions, but its conductivity increases with the addition of an electrolyte.

Experiment

1. Aim: To observe the process of electrolysis using a copper sulphate solution and understand the reactions at the cathode and anode.

2. Requirements: Copper sulphate solution (1 g CuSO₄ in 50 ml water), 100 ml beaker, copper plate (anode), carbon rod (cathode), power source (battery), electric circuit with a switch and wires.

3. Procedure:

  • Prepare a copper sulphate solution by dissolving 1 g of CuSO₄ in 50 ml of water in a beaker.
  • Immerse a copper plate (anode) and a carbon rod (cathode) in the solution.
  • Connect the copper plate to the positive terminal of the battery and the carbon rod to the negative terminal.
  • Turn on the electric current and let it flow through the circuit for some time.
  • Observe the changes occurring at the cathode and anode.

Electrolysis

4. Observations: Copper deposits appear on the carbon rod (cathode). The colour of the solution remains the same throughout the process.

5. Conclusion: At the cathode, Cu²⁺ ions from the solution gain electrons and form copper atoms, depositing on the electrode

Cu²⁺ (aq) + 2e⁻ → Cu (s)

At the anode, copper atoms from the copper plate lose electrons to form Cu²⁺ ions, which enter the solution:

Cu (s) → Cu²⁺ (aq) + 2e⁻

The solution's colour remains unchanged because the number of Cu²⁺ ions entering the solution at the anode equals those being deposited at the cathode.

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Related QuestionsVIEW ALL [90]

108 g of silver (molar mass 108 g mol-1) is deposited at cathode from AgNO3 (aq) solution by a certain quantity of electricity. The volume (in L) of oxygen gas produced at 273 K and 1 bar pressure from water by the same quantity of electricity is ______.

Element X is a metal with a valency 2. Element Y is a non-metal with a valency 3.

If the compound formed between X and Y is melted and an electric current passed through the molten compound, the element X will be obtained at the ______ and Y at the ______ of the electrolytic cell. (Provide the missing words).

Write equations for the reactions taking place at the two electrodes (mentioning clearly the name of the electrode) during the electrolysis of Acidified copper sulphate solution with copper electrodes

Choose the correct answer from the option given below:
Which one is weak electrolyte?

Explain, why electrolysis is an example of redox reaction?

Write the equation taking place at the anode

Give reason for the following:

In the electrolysis of acidified water, dilute sulphuric acid is preferred to dilute nitric acid for acidification.

Electrolysis is the passage of ______ through a liquid or a solution accompanied by a ______ change.

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