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Secondary 4 Pure Chemistry Redox Electrochemistry Quiz

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Secondary 4 Pure Chemistry AI Generated Generated by Gemma 4 31B Updated 2026-06-03

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Secondary 4 Pure Chemistry Quiz - Redox Electrochemistry

Name: ____________________
Class: ____________________
Date: ____________________
Score: ________ / 50

Duration: 60 Minutes
Total Marks: 50

Instructions:

Answer all questions in the spaces provided.
Show all working for calculations.
State symbols must be included in chemical equations where required.
Use a ruler for any diagrams.

Section A: Fundamentals of Redox (Questions 1–7)

Define "oxidation" in terms of electron transfer. [1]
\
In the reaction: $\text{CuO(s)} + \text{H}_2\text{(g)} \rightarrow \text{Cu(s)} + \text{H}_2\text{O(l)}$ , identify the reducing agent. [1]
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Assign oxidation numbers to the underlined elements in the following compounds: [2] (a) $\underline{\text{Mn}}\text{O}_4^-$ : ___________ (b) $\text{K}_2\underline{\text{Cr}}_2\text{O}_7$ : ___________
A student adds potassium manganate(VII) solution to a solution containing $\text{Fe}^{2+}$ ions. (a) State the color change observed. [1] \

(b) Explain this observation in terms of redox. [2]
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Write the ionic half-equation for the oxidation of $\text{Zn}$ to $\text{Zn}^{2+}$ . [1]
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Which of the following is a strong oxidizing agent? [1] A) $\text{Na}$ B) $\text{Mg}$ C) $\text{Cl}_2$ D) $\text{I}_2$ \
Explain why the reaction between $\text{Mg}$ and $\text{CuSO}_4$ is a redox reaction. [2]
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Section B: Electrolysis (Questions 8–14)

State the function of the electrolyte in an electrolytic cell. [1]
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During the electrolysis of molten lead(II) bromide ( $\text{PbBr}_2$ ): (a) Name the product formed at the cathode. [1] \

(b) Describe the observation at the anode. [1] \
In the electrolysis of concentrated aqueous sodium chloride: (a) Which gas is evolved at the anode? [1] \

(b) Write the half-equation for the reaction occurring at the cathode. [2]
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Explain why hydrogen gas is produced at the cathode instead of sodium metal during the electrolysis of dilute aqueous $\text{NaCl}$ . [2]
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A piece of graphite is used as an electrode in the electrolysis of aqueous $\text{CuSO}_4$ . (a) Why is graphite preferred over a reactive metal like iron? [1] \

(b) State the observation at the anode. [1] \
Describe the process of electroplating a copper spoon with silver. Include the identity of the anode, cathode, and electrolyte. [3]
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In the purification of copper, an impure copper anode is used. Explain why the anode decreases in mass over time. [2]
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Section C: Chemical Cells & Fuel Cells (Questions 15–20)

In a simple electrochemical cell consisting of a zinc strip and a copper strip in their respective sulfate solutions: (a) Which metal acts as the anode? [1] \

(b) In which direction do electrons flow through the external wire? [1] \
Write the half-equation for the reduction of $\text{Cu}^{2+}$ ions at the cathode in a $\text{Zn-Cu}$ cell. [1]
\
Explain the role of a salt bridge in a galvanic cell. [2]
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A hydrogen fuel cell is used to power a vehicle. (a) State the two reactants used in the fuel cell. [1] \

(b) State the only product formed by the reaction. [1] \
Write the overall balanced equation for the reaction occurring in a hydrogen fuel cell. [2]
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Compare a hydrogen fuel cell with a traditional combustion engine in terms of environmental sustainability. [3]
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Answers

Answer Key - Redox Electrochemistry Quiz

1. Oxidation is the loss of electrons. (1m)

2. $\text{H}_2$ (or Hydrogen). (1m) - It removes oxygen from $\text{CuO}$ .

3. (a) $+7$ (1m) (b) $+6$ (1m)

4. (a) Purple to colorless. (1m) (b) $\text{MnO}_4^-$ is reduced to $\text{Mn}^{2+}$ (colorless) while $\text{Fe}^{2+}$ is oxidized to $\text{Fe}^{3+}$ . (2m)

5. $\text{Zn(s)} \rightarrow \text{Zn}^{2+}\text{(aq)} + 2\text{e}^-$ (1m)

6. C) $\text{Cl}_2$ (1m)

7. $\text{Mg}$ is oxidized (loses electrons) and $\text{Cu}^{2+}$ is reduced (gains electrons). (2m)

8. To allow the movement of ions to complete the circuit / conduct electricity. (1m)

9. (a) Lead (Pb). (1m) (b) Red-brown fumes of bromine gas evolved. (1m)

10. (a) Chlorine gas ( $\text{Cl}_2$ ). (1m) (b) $2\text{H}^+\text{(aq)} + 2\text{e}^- \rightarrow \text{H}_2\text{(g)}$ . (2m)

11. $\text{H}^+$ ions are lower in the reactivity series (easier to reduce) than $\text{Na}^+$ ions, so $\text{H}^+$ is selectively discharged. (2m)

12. (a) Graphite is inert and will not react with the electrolyte/products. (1m) (b) Bubbles of oxygen gas evolved. (1m)

13.

Anode: Pure silver ( $\text{Ag}$ ) electrode. (1m)
Cathode: Copper spoon. (1m)
Electrolyte: Silver nitrate ( $\text{AgNO}_3$ ) solution. (1m)

14. Impure copper atoms at the anode are oxidized to $\text{Cu}^{2+}$ ions and enter the solution. (2m)

15. (a) Zinc ( $\text{Zn}$ ). (1m) (b) From Zinc (anode) to Copper (cathode). (1m)

16. $\text{Cu}^{2+}\text{(aq)} + 2\text{e}^- \rightarrow \text{Cu(s)}$ (1m)

17. It maintains electrical neutrality by allowing ions to migrate between the two half-cells. (2m)

18. (a) Hydrogen ( $\text{H}_2$ ) and Oxygen ( $\text{O}_2$ ). (1m) (b) Water ( $\text{H}_2\text{O}$ ). (1m)

19. $2\text{H}_2\text{(g)} + \text{O}_2\text{(g)} \rightarrow 2\text{H}_2\text{O(l)}$ (2m)

20.

Fuel cells produce only water, whereas combustion engines produce $\text{CO}_2$ and $\text{NO}_x$ (greenhouse gases/pollutants). (2m)
Fuel cells are more efficient/cleaner. (1m)