Suppose a $500.mL$ flask is filled with $0\mathrm{.}20$mol of $N{O}_2,0\mathrm{.}30$mol of $CO$ and $2\mathrm{.}0$mol of $NO.$ The following reaction becomes possible:

$N{O}_2(g)+CO(g)NO(g)+C{O}_2(g)$

The equilibrium constant $K$ for this reaction is $0\mathrm{.}836$ at the temperature of the flask.

Calculate the equilibrium molarity of $N{O}_2.$ Round your answer to two decimal places.