An electrochemical cell is made by combining two half cells

$\overline{){\mathrm{AgNO}}_3\left(0.05\right)\mathrm{M}}\mathrm{Ag}\left(\mathrm{s}\right)$ and $\left(\mathrm{Y}\right)$ $\overline{)\left.{\mathrm{AgNO}}_3\left(0.01\right)\mathrm{M}\right)}\mathrm{Ag}\left(\mathrm{s}\right)$

Choose the correct statement

Which of the following expression(s) represent the voltage of cell at $298 \mathrm{K}$?

$\mathrm{Ag}\left(\mathrm{s}\right)|\underset{\begin{array}{l}\left(1\right) \mathrm{saturated}\\ \mathrm{solution}\end{array}}{\mathrm{AgI}}\underset{\begin{array}{l}\left(2\right) \mathrm{saturated}\\ \mathrm{solution}\end{array}}{\left|\right|{\mathrm{Ag}}_2{\mathrm{C}}_2{\mathrm{O}}_4 |}\mathrm{Ag}\left(\mathrm{s}\right)$

In the following electrochemical cell: $\mathrm{Pt} \overline{) {\mathrm{H}}_2} \left(\mathrm{x} \mathrm{atm}\right) \overline{) {\mathrm{H}}^{+} }\left(\mathrm{pH}=\mathrm{y}\right) \Vert {\mathrm{Zn}}^{2+} \left(\mathrm{z} \mathrm{M}\right) \overline{) \mathrm{Zn}}$

${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}={\mathrm{E}}_{\text{cell }}.$ This will be possible when

The cell potential for the unbalanced chemical reaction :

${\mathrm{Hg}}_2^{2+}+{\mathrm{NO}}_3^{-}+{\mathrm{H}}^{+}⟶{\mathrm{Hg}}^{2+}+{\mathrm{HNO}}_2+{\mathrm{H}}_2\mathrm{O};{\mathrm{E}}_{\mathrm{cell} }^{\mathrm{o}}=0.02 \mathrm{V}$

$\left(\frac{2.303\mathrm{RT}}{F}=0.06\right)$

Then choose the correct statement.