For the second-order reaction, 2A rightarrow B + C, it is found that 15% of the sample has reacted in 12 seconds when [A]_o = 0.30 M. Determine the rate constant and half-life for this reaction. A certain reaction was studied and it was determined that 1/16 of the original reactant remained. Determine the time required if the reaction was first-order with t_1/2 = 20 sec. second-order with t_1/2 = 20 sec. The gas-phase decomposition or SO_2 Cl_2 follows the equation, SO_2 Cl_2 rightarrow SO_2 Cl_2. The reaction is first-order with a rate constant of 2.2 times 10^-5 s^-1 at 320 degree C. If the initial concentration of SO_2 Cl_2 in a container is 0.0060 M, what will its concentration be after 1.00 hour? after 1.00 day? Suppose that a certain first order reaction has a half-life of 12.0 sec. How many seconds are required for the concentration of the reactant to change from 0.40 M to 0.05 M? For the gas-phase reaction, 2NO + O_2 rightarrow 2NO_2, the experimental (differential) rate law is r = k(NO]^2 [O_2]. Is the following mechanism consistent with the rate law? NO + O_2 NO_3 FAST equilibrium step NO_3 + NO rightarrow 2NO_2 SLOW