The gas phase decomposition of dinitrogen pentoxide is represented by this equation, 

$2{\mathrm{N}}_2{\mathrm{O}}_5\left(g\right)⟶4{\mathrm{NO}}_2\left(g\right)+{\mathrm{O}}_2\left(g\right)$

What is the rate of formation of oxygen gas (in $\left.\mathrm{mol}\cdot \mathbf{L}\cdot {\mathrm{s}}^{-1}\right)$ in an experiment where 0.080 mol of ${\mathrm{N}}_2{\mathrm{O}}_5$ is consumed in a 4.0 L container every 0.20 seconds?