1. Tardigrade
  2. Question
  3. Chemistry
  4. All the energy released from the reaction X → Y, ΔrGº = -193 kJ mol- is used for oxidizing M+ as M+ → M3+ + 2e-, Eº = -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 mol-1]

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Q. All the energy released from the reaction $X → Y, ΔrGº = -193 \,kJ \,mol^-$ is used for oxidizing $M^+$ as $M^+ → M^{3+} + 2e^-, Eº = -0.25\, V$. Under standard conditions, the number of moles of $M^+$ oxidized when one mole of X is converted to Y is
$[F = 96500\, C \,mol^{-1}]$

JEE AdvancedJEE Advanced 2015

Solution:

$M^{+} → M^{3+} + 2e^{-}$
$nM^{+} → nM^{3+} + 2ne^{-}\quad ΔGº = -2n\, FEº$
And :
$|ΔrGº| = |ΔGº|$
$∴ 193 × 1000 = 2 × n × 96500 × 0.25$
$n = 4$