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Given the following reactions and standard electrode potentials: 1. 2Cu⁺ → Cu²⁺ + Cu 2. 2e⁻ + Cu²⁺ → Cu; E°₁ = 0.34V 3. E°₂ = 0.15V For the reaction Cu⁺ + e⁻ → Cu²⁺, calculate E°₃ using the relationship ΔG° = -n × E°F. If E°₃ = 0.53 - 0.15, what is the value of E°₃?

1. E°₁ = 0.34V
2. E°₂ = 0.15V
3. E°₃ = 0.38V
4. ΔG°₁ = -n × 0.15F

Correct answer: E°₃ = 0.38V

Solution

The question involves calculating the standard electrode potential (E°₃) for the reaction Cu⁺ + e⁻ → Cu²⁺. Using the given data and the relationship between Gibbs free energy and electrode potential, E°₃ is correctly calculated as 0.38V.

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