Consider the equilibrium reaction:

$2N_2(g)+O_2(g)2N_{2}O(g)$

In a particular experiment, the equilibrium concentration of $N_2$ is $0\mathrm{.}048$ molar, of $O_2,0\mathrm{.}093$ molar, and of $N_{2}O$ is $6\mathrm{.}55{10}^{-8}$ molar. What is the value of the equilibrium constant $K?$

$6.$ A $3\mathrm{.}00-$liter flask initially contains $1\mathrm{.}50$mol of gas A and $0\mathrm{.}850$mol of gas B$.$ Gas A decomposes according to the following reaction:

$3A2B+C$

The equilibrium concentration of gas $C$ is $0\mathrm{.}131mo\frac{l}{L}.$ Determine the value of the equilibrium constant, $K.$