NO and O₂ react to form NO₂ at 298K according to the reaction.
${\mathrm{NO}}_{\left(\mathrm{g}\right)}+\frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{NO}}_{2\left(\mathrm{g}\right)}$
Initially pressure of NO and O₂ are 1 atm and 11/4 atm respectively and the final pressure of NO is x × 10^-8atm. The value of x is _______. [Use (10^6.13 = 1.34 x 10⁶)]
(Given: ${\mathrm{\Delta G}}_{\mathrm{f}}^{\mathrm{o}}{\left({\mathrm{NO}}_2\right)}_{\left(\mathrm{g}\right)}=52 \mathrm{KJ}/\mathrm{mol},{\mathrm{\Delta G}}_{\mathrm{f}}^{\mathrm{o}}(\mathrm{NO}{)}_{\left(\mathrm{g}\right)}=$87 KJ/mol ) (report the value to nearest
integer)