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In the reaction X → Y, where ΔG° = -193 kJ mol⁻¹, all the energy released is utilized to oxidize M⁺ to M³⁺ according to the equation M⁺ → M³⁺ + 2e⁻, with E° = -0.25 V. Under standard conditions, how many moles of M⁺ are oxidized when one mole of X transforms into Y? [F = 96500 C mol⁻¹]
- 1 mole
- 2 moles
- 3 moles
- 4 moles
Correct answer: 4 moles
Solution
The energy released in the reaction X → Y is used to oxidize M⁺ to M³⁺. Using ΔG = -nFE° and substituting the given values, the number of moles of M⁺ oxidized is calculated as 4 moles.
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