Nitrogen and oxygen do not react appreciably at room tempera

Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. But at high temperatures, the reaction below can proceed to a measurable extent.
N₂(g) + O₂(g) ⇔ 2 NO(g)
At 3000 K, the reaction above has K_eq = 0.0153. If 0.3152 mol of pure NO is injected into an evacuated 2.0-L container and heated to 3000K, what will be the equilibrium concentration of NO?

Solution

Oh sorry i made a small mistake last time,Actually K = [NO]^2 / [N2]*[O2], so 0.0153 = [(0.3152 - 2x)/2]^2 /x/2 *x/2 , so x = 0.1484, so at equilibrium conc. of NO is( 0.3152 - 2x )/2 = 9.2*10^-3