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All the energy released from the reaction X ⟶ Y ,   Δ r G o = - 193   k J   m o l - 1 is used for oxidizing M + as M + ⟶ M 3 + + 2 e -   ,   E o =   - 0.25   V Under standard conditions, the number of moles of M + oxidized when one mole of X is converted to Y is [ F = 96500   C   m o l - 1 ]

Correct answer

4

Step-by-step solution

M + → M 3 + + 2 e - ∆ G o = - n F E o for 1 mole of M + ∆ G o = - 2 × 96500 × - 0.25 J = + 48250 J/mole = 48.25   K J /mole Energy released by conversion of 1 mole of X → Y ∆ G = - 193   K J Hence mole of M + convert 193 48.25 = 4  

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