Copper reduces $\mathrm{NO}_3^{-}$into NO and $\mathrm{NO}_2$ depending upon the concentration of $\mathrm{HNO}_3$ in solution. (Assuming fixed $\left[\mathrm{Cu}^{2+}\right]$ and $\mathrm{P}_{\mathrm{NO}}=\mathrm{P}_{\mathrm{NO} 2}$ ), the $\mathrm{HNO}_3$ concentration at which the thermodynamic tendency for reduction of $\mathrm{NO}_3^{-}$into NO and $\mathrm{NO}_2$ by copper is same is $10^x \mathrm{M}$. The value of 2 x is
$\_\_\_\_$ (Rounded-off to the nearest integer)
$$
\begin{aligned}
&\text { [Given, }\\
&\begin{aligned}
& \mathrm{E}_{\mathrm{Cu}^{2 .} / \mathrm{Cu}}^{\circ}=0.34 \mathrm{~V}, \mathrm{E}_{\mathrm{NO}_3^{-} / \mathrm{NO}}^{\circ}=0.96 \mathrm{~V}, \\
& \mathrm{E}_{\mathrm{NO}_3^{-} / \mathrm{NO}_2}^{\circ}=0.79 \mathrm{~V} \text { and at } 298 \mathrm{~K}, \\
& \left.\qquad \frac{\mathrm{RT}}{\mathrm{~F}}(2.303)=0.059\right]
\end{aligned}
\end{aligned}
$$