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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, we need to determine how many moles of \( M^+ \) can be oxidized when 1 mole of \( X \) is converted to \( Y \), given that the reaction releases \( \Delta_r G^\circ = -330.03 \, \text{kJ/mol} \). ### Step-by-Step Solution: 1. **Understand the Energy Released**: The energy released from the conversion of 1 mole of \( X \) to \( Y \) is given as \( -330.03 \, \text{kJ/mol} \). This energy will be used to oxidize \( M^+ \). 2. **Calculate the Energy Required to Oxidize 1 Mole of \( M^+ \)**: ...
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