For the following reaction:

$\mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)⟶2\mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$

the rate law is given as rate of disappearance A =$\mathrm{K}\left[\mathrm{A}{]}^{2/3}\right[\mathrm{B}{]}^{1/3}$. If initial concentration of A and B are 2M each and no C and D were present initially, then the time at which total concentration (sum of concentrations of A, B, C and D) will become 5.5 M, is:

(Given:$\mathrm{K}=1.386\times {10}^{-1}{\min }^{-1}$)