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SS2: CHEMISTRY - 1ST TERM

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  1. Periodicity and Periodic Table I | Week 1
    5 Topics
    |
    1 Quiz
  2. Quantum Numbers Orbitals & Electrical Structure | Week 2
    6 Topics
    |
    1 Quiz
  3. Periodicity and Periodic Table II | Week 3
    12 Topics
    |
    1 Quiz
  4. Periodicity and Periodic Properties III | Week 4
    11 Topics
    |
    1 Quiz
  5. Periodicity and Periodic Properties IV | Week 5
    5 Topics
    |
    1 Quiz
  6. Mass-Volume Relationship in Reaction | Week 6
    8 Topics
    |
    1 Quiz
  7. Types of Reactions: Oxidation and Reduction | Week 7 & 8
    7 Topics
    |
    1 Quiz
  8. Oxidation – Reduction Reaction II | Week 9
    3 Topics
    |
    1 Quiz
  9. Electrode Potential and Electrochemical Cells I | Week 10
    6 Topics
    |
    1 Quiz
  10. Electrode Potential and Electrochemical Cells II | Week 11
    5 Topics
    |
    1 Quiz
  11. Electrolysis I | Week 12
    8 Topics
    |
    1 Quiz
  12. Electrolysis II | Week 13
    8 Topics
    |
    1 Quiz

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SS2: CHEMISTRY – 1ST TERM Electrolysis I | Week 12 Theory Questions – Electrolysis
Lesson 11, Topic 8
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Theory Questions – Electrolysis

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Topic Content:

  • Theory Questions and Answers – Electrolysis

Theory Questions – Electrolysis:

1.  (a) What is a conductor? Give two examples of a conductor

(b) Classify the following as conductor/non-conductor. 

 (i) Iron rod     (ii) Candle     (iii) Tin can      (iv) Rubber       (v) Diamond  

2.  What is an electrolyte? Give two examples of electrolyte

(b) Define a non-electrolyte 

(c) Explain why NaCl(s) does not conduct electricity, but NaCl(aq) does

3.  Write the equations for anodic and cathodic half-reactions which occur during electrolysis of copper(II) tetraoxosulphate(IV) solutions, using the following electrodes 

(i) Platinum electrodes

(ii) copper electrodes 

(iii) Copper cathode and carbon anode 

(iii) Carbon cathode and copper anode

(b) List three factors affecting the discharge of ions in electrolysis. 

4. Which of the following ions will migrate to the Cathode during electrolysis?

 (a) Zinc ions

(b) Chloride ions

(c) Sulphide ions

(d) Tetraoxosulphate(vi)ions

5.   (a) Define the term electrolysis. 

(b) (i) What are electrodes? (ii) Name two types of electrodes.

(c) Distinguish between the anode and the cathode 

(d) Draw and label a simple electrolytic cell

6.  (a) State and explain how the pH of the electrolyte changes during the electrolysis of dilute CuCl2(aq) using graphite electrodes.

(b) List the ions present in the aqueous solution of iron(II) tetraoxosulphate(VI)

(c) With the aid of a well-labeled diagram describe the electrolysis of dilute sodium tetraoxosulphate(VI) using suitable electrodes. Name the electrodes

 

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Evaluation Questions

1.  (a) What is a conductor ? Give two examples of a conductor

Answer:

Conductors are substances which contain mobile electrons and allow the passage of electricity without decomposition. 

e.g. metals, graphite

 

(b) Classify the following as conductor/non-conductor

(i) Iron rod     (ii) Candle     (iii) Tin can      (iv) Rubber       (v) Diamond

Answer –  

i. Iron rod – conductor

ii. Camole – Non conductor

iii. Tin can – conductor

iv. Rubber – Non-conductor

v. Diamond – Non-conductor

 

2a  What is an electrolyte? Give two examples of electrolyte

Answer:  An electrolyte is a compound in the solution or molten form which conducts electric current with decomposition at the electrode e.g. acids, alkali

 

(b) Define a non-electrolyte

Answer –  Non-electrolyte is a compound in solution or molten form which does not allow the passage of electricity.

 

(c) Explain why NaCl(s) does not conduct electricity, but NaCl(aq) does

Answer – 

NaCl(s) does not conduct electricity because it is in solid form.

NaCl(aq) conducts electricity because it is in aqueous form

 

3.  Write the equations for anodic and cathodic half-reactions which occur during electrolysis of copper(II) tetraoxosulphate(IV) solutions, using the following electrodes

(i) Platinum electrodes 

Answer:

CuSO4(aq) ⇌ Cu2+(aq) + SO42-(aq)

H2O(l)  ⇌ H+(aq)+ OH–(aq)

At the cathode

Cu2+ + 2e–  → Cu(s)

At the anode

OH– →  OH + e– 

OH + OH →  H2O + O2

O + O  →  O2(g)

(ii) copper electrodes

Answer:

Cathode half  =  Cu2+(aq)  +  2e–  →  Cu(s)

Anode half = Cu(s) → Cu2+(aq)  +  2e– 

(iii) Copper cathode and carbon anode

Answer:

Cathode half  =  Cu2+(aq)  +  2e–  →  Cu(s)

At the anode

OH– →  OH + e– 

OH + OH →  H2O + O2

O + O  →  O2(g)

(iv) Carbon cathode and copper anode

Answer:

Cathode half  =  Cu2+(aq)  +  2e–  →  Cu(s)

Anode half = Cu(s) → Cu2+(aq)  +  2e– 

 

(b) List three factors affecting the discharge of ions in electrolysis.

Answer:

i) Concentrate of ions in the electrolyte

ii) Nature of the electrode

iii) Position of ions in electrochemical series

 

4. Which of the following ions will migrate to the Cathode during electrolysis?

(a) Zinc ions

(b) Chloride ions

(c) Sulphide ions

(d) Tetraoxosulphate(vi)ions

Answer:  Zinc ions

 

5.   (a) Define the term electrolysis

Answer:  Electrolysis is the chemical decomposition of a compound brought about by a direct current passing through it either in solution or molten form of the compound.

 

(b) (i) What are electrodes? 

Answer:  Electrodes are conductors through which current enters or leaves the electrolyte.

 

(ii) Name two types of electrodes.

Answer:

Anode

Cathode

 

(c) Distinguish between the anode and the cathode

Answer – 

The anode is a positive electrode by which current enters the electrolyte.

The cathode is a negative electrolyte by which current leaves the electrolyte.

 

(d) Draw and label a simple electrolytic cell

Answer – 

 

6.  (a) State and explain how the pH of the electrolyte changes during the electrolysis of dilute CuCl2(aq) using graphite electrodes.

(b) List the ions present in the aqueous solution of iron(II) tetraoxosulphate (VI)

Answer:

Fe2+ + SO42-

H+  OH–

 

(c) With the aid of a well-labelled diagram, describe the electrolysis of dilute sodium tetraoxosulphate(VI) using suitable electrodes. Name the electrodes

Answer – 

At the cathode

2H+ → H2  +  2e– 

At the anode

OH– →  OH + e 

OH + OH →  H2O + O2

O + O  →  O2(g)

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