Discussion Forum

1)

 All the energy released  from the reaction

   $X\rightarrow Y,\triangle_{r}G^{0}=-193kJmol^{-1}$

  is used for oxidising  M⁺ as   $M^{+}\rightarrow M^{3+}+2\overline{e}$, E⁰  =-0.25 V.

 Under standard conditions , the number of moles  of M⁺ oxidised  when one mole of X is converted to Y  is [F=96500 C mol^-]

Answer:

Option A

Explanation:

Energy obtained as one mole X is converted into Y is 193 KJ

Energy consumed in converting  one mole of M⁺ to M³⁺

      $= -nE^{0}F=2\times96500\times0.25 J=\frac{96500}{2}J$

   $\Rightarrow193\times10^{3}=n\left(\frac{96500}{2}\right)$

  $\Rightarrow$               n=4 mol