For the following electrochemical cell at 298 K , $$ \begin{aligned} & \operatorname{Pt}(\mathrm{s}) \mid \mathrm{H}_2(\mathrm{~g}, 1 \text { bar })\left|\mathrm{H}^{+}(\mathrm{aq}, 1 \mathrm{M})\right|\left|\mathrm{M}^{4+}(\mathrm{aq}), \mathrm{M}^{2+}(\mathrm{aq})\right| \operatorname{Pt}(\mathrm{s}) \\ & \mathrm{E}_{\text {cell }}=0.092 \mathrm{~V} \text { when } \frac{\left[\mathrm{M}^{2+}(\mathrm{aq})\right]}{\left[\mathrm{M}^{4+}(\mathrm{aq})\right]}=10^{\times} \end{aligned} $$ Given : $\mathrm{E}_{\mathrm{M}^{4+} / \mathrm{M}^{2+}}^0=0.151 \mathrm{~V} ; 2.303 \frac{\mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{~V}$ The value of $x$ is