(Solved): A 100mL reaction vessel initially contains 2.60102 moles of NO and 1.30102 moles of H2 ...

A $100?\mathrm{mL}$ reaction vessel initially contains $2.60\times 10^{?2}$ moles of $\mathrm{NO}$ and $1.30\times 10^{?2}$ moles of ${\mathrm{H}}_2$. At equilibrium, the concentration of NO in the vessel is $0.161\mathrm{M}$. At equilibrium the vessel also contains ${\mathrm{N}}_2,{\mathrm{H}}_2\mathrm{O}$, and ${\mathrm{H}}_2$. What is the value of the equilibrium constant $\mathrm{Kc}$ for the following reaction? $2{\mathrm{H}}_2(g)+2\mathrm{NO}(\mathrm{g})?2{\mathrm{H}}_2\mathrm{O}(g)+{\mathrm{N}}_2(g)$