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All the energy released from the reactio...

All the energy released from the reaction `Xto Y`, `Delta_(r) G^(@) = -330.03KJ//mol` is used for of moles of `M ^(+)` oxidisesd when one mol of X is converted to Y is:` (F= 96500Cm1^(-1)`)

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To solve the problem step by step, we will use the relationship between Gibbs free energy change (ΔG°), Faraday's constant (F), and the cell potential (E°) to find the number of moles of M^+ oxidized when one mole of X is converted to Y. ### Step 1: Write down the Gibbs free energy equation The relationship between Gibbs free energy change and the cell potential is given by the equation: \[ \Delta G = -nFE^\circ \] where: ...
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All the energy released from the reaction XtoY,Delta _(r)G^(@) = -193KJmol^(-1) is used for oxidizing M^(+) as M^(+)toM^(3+)+ 2e^(-) , e^(@) =-0.25V . Under standard conditions, the number of moles of oxidized when one mole of X is converted to Y is [F = 96500Cmol^(-1)]

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