The mechanism of a reaction A → B is investigated. At the beginning of the reaction, the concentration of A is 1.91 ✕ 10−3 M. After 75.6 s, the concentration of A is 4.98 ✕ 10−5 M. Using the integrated rate laws, calculate the half-life of the reaction at 75.6 s for the following conditions.
(a) The reaction is first order in A.
(b) The reaction is second order in A.
Consider the following first-order reaction: A → B. The concentration of A at the start of the reaction is 4.18 M and after 4.95 s is 3.57 M.
(a) Using the integrated rate law for a first-order reaction, calculate the value of the rate constant.
(b) Calculate the half-life of the reaction.
