A constant volume batch reactor was used to study the reversible, liquid-phase isomerization reaction of compound B going to compound T, ie the two reactions are (1) B -->T and (2) T->B. The reactions are both first order. Compounds T and B are both initially present in the reactor, with an initial concentration of T of 67.5 mol/L and of B of 14.7 mol/L. At 20C, the equilibrium conversion of compound B is 91%. The rate constants of the forward reaction (i.e. reaction 1) is 0.88 hour. How long (in minutes) will it take for the conversion of B to reach 30%? Express your answer in minutes, to one decimal place.