Given at 298 K :

$$ \begin{aligned} & \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\ominus}=\mathrm{X} \text { Volt } \\ & \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}}^{\ominus}=\mathrm{Y} \text { Volt } \end{aligned} $$

The $\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\ominus}$ in Volt at 298 K is given by :

For a general redox reaction

Anode $\quad \operatorname{Red}_1 \rightarrow \mathrm{Ox}_1^{\mathrm{n}_1^{+}}+\mathrm{n}_1 \mathrm{e}^{-}$

Cathode $\mathrm{O} x_2+\mathrm{n}_2 \mathrm{e}^{-} \rightarrow \operatorname{Red}_2^{\mathrm{n}_2-}$

Which of the following statement is incorrect?

$$ \text { Consider the following data. } $$

$$ \begin{array}{|c|c|} \hline \text { Electrolyte } & \wedge^{\circ}_\mathbf{m}{\mathbf{(}} \mathbf{S ~ c m}^{\mathbf{2}} \mathbf{~ m o l}^{\mathbf{1}} \mathbf{)} \\ \hline \mathrm{BaCl}_2 & x_1 \\ \hline \mathrm{H}_2 \mathrm{SO}_4 & x_2 \\ \hline \mathrm{HCl} & x_3 \\ \hline \end{array} $$

$\mathrm{BaSO}_4$ is sparingly soluble in water. If the conductivity of the saturated $\mathrm{BaSO}_4$ solution is $x \mathrm{~S} \mathrm{~cm}^{-1}$ then the solubility product of $\mathrm{BaSO}_4$ can be given as (Here $\wedge_{\mathrm{m}}=\wedge^{\circ}_{\mathrm{m}}$ )

One half cell in a voltaic cell is constructed by dipping silver rod in $\mathrm{AgNO}_3$ solution of unknown concentration, other half cell is Zn rod dipped in 1 molar solution of $\mathrm{ZnSO}_4$.

A voltage of 1.60 V is measured at 298 K for this cell. What is the concentration of $\mathrm{Ag}^{+}$ions used in terms of $\log x\left(x=\left[\mathrm{Ag}^{+}\right]\right)$?

$$ \mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{\ominus}=-0.76 \mathrm{~V}, \quad \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\ominus}=+0.80 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{~F}}=0.059 \mathrm{~V} $$