The gas phase decomposition of dimethyl ether at 500 °C CH3OCH3(g) → CH4 (g) + H2 (g) + CO (g) is first order in CH3OCH3 with a rate constant of 4.00×10-4 s-1 How much time in seconds is required for 85.2% of the CH3OCH3 initially present in a reaction flask to be converted to product at this temperature? (enter a numerical value, don't worry about the units, put exponents as e#. For example, 4.00×10-4 would be 4.00e-4)