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)]`

Explanation

To solve the problem, we need to determine how many moles of \( M^+ \) are oxidized when one mole of \( X \) is converted to \( Y \). We will use the provided values for \( \Delta G \) and the standard reduction potential \( E^\circ \).

### Step-by-Step Solution:

1. **Identify Given Values**:
- \( \Delta G^\circ = -193 \, \text{kJ/mol} \)
- \( E^\circ = -0.25 \, \text{V} \)
- Faraday's constant, \( F = 96500 \, \text{C/mol} \)
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