You are studying the rate of the reaction 2A → B and have obtained measurements of the concentration of A attimes t = 100, 200, 300, ......, 1000 seconds from the start of the reaction. Carefully describe how you would plot agraph and use it to:a) prove that the reaction is second-order with respect to A.b) determine the second-order rate constant k.

A chemical reaction of the general type:   A → 2B is first-order, with a rate constant of 1.52 × 10-4 s-1. a) Calculate the half-life of A. b) Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.

23. The rate constant for decomposition of azomethane at 425°C is 0.68 s~', CH,N=NCH,(g) N;(g) + C,H(g) a) Based on the units of the rate constant, is the reaction zeroth-, first-, or second-order? b) If2.0 g azomethane is placed in a 2.0-L flask and heated to 425°C, what mass of azomethane remains after 5.0 s? c) How long does it take for the mass of azomethane to drop to 0.24 g? d) What mass of nitrogen would be found in the flask after 0.50 s of reaction?

A reaction that is second-order in reactant A has [A]o = 0.200 M. The half-life is 45.6 sec. What is [A] after 3.00 min? Report the molarity in standard notation with 3 significant figures and do not include units (M).