1. Tardigrade
  2. Question
  3. Chemistry
  4. All the energy released from the reaction X arrow Y , Δ r G °=-193 kJ mol -is used for oxidizing M +as M + arrow M 3++2 e -, E °=-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]

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

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

Electrochemistry

Solution:

$M ^{+} \rightarrow M ^{3+}+2 e ^{-}$
$nM ^{+} \rightarrow nM ^{3+}+2 ne ^{-}\,\, \Delta G ^{\circ}=-2 n\, FE ^{\circ}$
And :
$\left|\Delta_ r G ^{\circ}\right|=\left|\Delta G ^{\circ}\right|$
$\therefore 193 \times 1000=2 \times n \times 96500 \times 0.25$
$n =4$