Electrochemistry - Result Question 105
53. All the energy released from the reaction $X \rightarrow Y, \Delta _r G^{\circ}=-193 $ $kJ $ $mol^{-1}$ is used for oxidising $M^{+}$ as $M^{+} \rightarrow M^{3+}+2 e^{-}, E^{\circ}=-0.25 V$.
Under standard conditions, the number of moles of $M^{+}$ oxidised when one mole of $X$ is converted to $Y$ is $[nF=96500 $ $C$ $ mol^{-1}]$
(2015 Adv.)
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Answer:
Correct Answer: 53. $(4 mol)$
Solution:
- Energy obtained as one mole $X$ is converted into $Y$ is $193 kJ$.
Energy consumed in converting one mole of $M^{+}$ to $M^{3+}$
$=-n E^{\circ} F=2 \times 96500 \times 0.25 J=3.86 \times 10^4 J$
$\Rightarrow 193 \times 10^{3} =n\left(\frac{96500}{2}\right) $
$\Rightarrow n=4$ $ mol$
BETA
