Electrochemistry Redox Applications

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🔋 Part 1: Redox Reactions and Half-Equations

1. In the reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

Zinc is reduced and copper is oxidised

Zinc is oxidised and copper is reduced

Both metals are oxidised

Both metals are reduced

2. Write the oxidation half-equation for the reaction above:

3. Write the reduction half-equation for the reaction above:

4. Which of these statements reflect Māori perspectives on transformation (Kaitiakitanga)? Select all that apply:

Chemical changes should be understood to protect our environment

Energy transformations connect all living and non-living things

We have responsibility as guardians of chemical processes

Natural cycles involve continuous transformation

⚡ Part 2: Cell Diagrams and Calculations

5. Complete this galvanic cell diagram for the zinc-copper cell:

Zn(s) | _________ || _________ | Cu(s)

6. In this cell diagram, which electrode is the anode?

Zinc electrode

Copper electrode

Salt bridge

Cannot be determined

7. Using the standard reduction potentials below, calculate E°cell for the zinc-copper cell:

Cu²⁺ + 2e⁻ → Cu E° = +0.34 V

Zn²⁺ + 2e⁻ → Zn E° = -0.76 V

E°cell = _______ V

8. Is this reaction spontaneous? Explain your reasoning:

🌱 Part 3: Real-World Applications

9. Explain how galvanic protection works to prevent corrosion of steel structures:

10. A Māori community wants to use sustainable battery technology for their marae. Suggest two electrochemical applications that align with Kaitiakitanga values and explain why:

11. Extension: Calculate the cell potential for this reaction under standard conditions:

Mg(s) + 2Ag⁺(aq) → Mg²⁺(aq) + 2Ag(s)

Ag⁺ + e⁻ → Ag E° = +0.80 V

Mg²⁺ + 2e⁻ → Mg E° = -2.37 V

Would this reaction be suitable for a battery? Explain: ________________________

Electrochemistry Redox Applications

Electrochemistry Redox Applications

🔋 Part 1: Redox Reactions and Half-Equations

⚡ Part 2: Cell Diagrams and Calculations

🌱 Part 3: Real-World Applications

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