Suppose a $500.mL$ flask is filled with $1\mathrm{.}9$mol of $O_2$ and $0\mathrm{.}50$mol of $NO.$ The following reaction becomes possible:

$N_2(g)+O_2(g)2NO(g)$

The equilibrium constant $K$ for this reaction is $4\mathrm{.}35$ at the temperature of the flask.

Calculate the equilibrium molarity of $N_2.$ Round your answer to two decimal places.