Secondary 3 Chemistry Redox Electrochemistry Quiz

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Secondary 3 Chemistry Quiz - Redox Electrochemistry

Name: ____________________
Class: ____________________
Date: ____________________
Score: ________ / 45

Duration: 60 Minutes
Total Marks: 45 Marks

Instructions:

• Answer all questions.
• For structured questions, write your answers in the spaces provided.
• Show all working for calculations.

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

1. Define oxidation in terms of oxygen gain/loss. [1] \

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2. Define reduction in terms of electron transfer. [1] \

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3. In the reaction $\text{CuO(s)} + \text{H}_2\text{(g)} \rightarrow \text{Cu(s)} + \text{H}_2\text{O(g)}$, identify the substance being reduced. [1] \

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4. State the oxidation state of the following species: [3] (a) $\text{K}$ in $\text{KCl}$: _________ (b) $\text{S}$ in $\text{H}_2\text{SO}_4$: _________ (c) $\text{Cr}$ in $\text{K}_2\text{Cr}_2\text{O}_7$: _________

5. Explain why a reaction is described as a redox reaction. [1] \

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6. Identify the oxidizing agent in the following reaction: [1] $\text{Zn(s)} + \text{CuSO}_4\text{(aq)} \rightarrow \text{ZnSO}_4\text{(aq)} + \text{Cu(s)}$ \

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7. Write a balanced chemical equation for the reaction between potassium iodide and chlorine water. [2] \

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Section B: Electrolysis of Molten and Aqueous Compounds (Questions 8–15)

8. Describe what happens at the anode during the electrolysis of molten lead(II) bromide. [2] \

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9. In the electrolysis of aqueous sodium chloride, why is hydrogen gas evolved at the cathode instead of sodium metal? [2] \

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10. Predict the products formed at the anode and cathode during the electrolysis of concentrated aqueous $\text{CuCl}_2$. [2] Anode: ____________________ Cathode: ____________________

11. Explain the term selective discharge in the context of aqueous electrolysis. [2] \

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12. During the electrolysis of aqueous $\text{AgNO}_3$ using copper electrodes, describe the change in mass of the anode. [2] \

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13. Write the half-equation for the reaction occurring at the cathode during the electrolysis of molten $\text{Al}_2\text{O}_3$. [2] \

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14. Why must the graphite electrodes in the electrolysis of aqueous $\text{NaCl}$ be inert? [1] \

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15. State the observation made at the cathode when aqueous $\text{ZnSO}_4$ is electrolyzed. [1] \

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Section C: Applications and Cells (Questions 16–20)

16. Describe the process of electroplating a steel spoon with silver. [3] \

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17. In the purification of copper, why is the impure copper used as the anode? [2] \

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18. Explain the role of the electrolyte in a simple chemical cell. [2] \

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19. A hydrogen fuel cell is used to power a vehicle. State the only product formed at the exhaust. [1] \

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20. Compare a simple chemical cell and an electrolytic cell in terms of energy conversion. [2] \

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Answer Key - Secondary 3 Chemistry Quiz: Redox Electrochemistry

1. Oxidation is the gain of oxygen. [1]

2. Reduction is the loss of electrons. [1]

3. $\text{CuO}$ (Copper(II) oxide). [1]

4. (a) +1; (b) +6; (c) +6. [3]

5. Because oxidation and reduction occur simultaneously in the same reaction. [1]

6. $\text{CuSO}_4$ (or $\text{Cu}^{2+}$ ions). [1]

7. $\text{Cl}_2\text{(g)} + 2\text{KI(aq)} \rightarrow 2\text{KCl(aq)} + \text{I}_2\text{(s/aq)}$. [2]

8. Negative bromide ions ($\text{Br}^-$) are attracted to the positive anode; they lose electrons (oxidation) to form brown bromine gas. [2]

9. Hydrogen ions ($\text{H}^+$) are lower in the reactivity series (or have a lower discharge potential) than sodium ions ($\text{Na}^+$), so $\text{H}^+$ is preferentially discharged. [2]

10. Anode: Chlorine gas ($\text{Cl}_2$); Cathode: Copper metal ($\text{Cu}$). [2]

11. The process where the ion with the lower discharge potential (or less reactive metal) is preferentially discharged at an electrode when multiple ions are present. [2]

12. The mass of the anode decreases as copper atoms lose electrons and enter the solution as $\text{Cu}^{2+}$ ions. [2]

13. $\text{Al}^{3+}\text{(l)} + 3\text{e}^- \rightarrow \text{Al(l)}$. [2]

14. To prevent the electrode from reacting with the products of electrolysis. [1]

15. A grey deposit of zinc metal forms on the electrode. [1]

16. The spoon is made the cathode; a pure silver rod is the anode; the electrolyte is a solution of silver ions (e.g., $\text{AgNO}_3$). $\text{Ag}^+$ ions move to the spoon and are reduced to $\text{Ag}$ metal. [3]

17. The impure copper anode dissolves (oxidizes) into the solution, allowing pure copper to deposit at the cathode. [2]

18. It allows the flow of ions to complete the circuit and maintain electrical neutrality. [2]

19. Water ($\text{H}_2\text{O}$). [1]

20. Simple cell: Chemical energy $\rightarrow$ Electrical energy. Electrolytic cell: Electrical energy $\rightarrow$ Chemical energy. [2]