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A reactant decomposes with a half-life of 193 s when its initial concentration is 0.203 m. when the initial concentration is 0.540 m, this same reactant decomposes with the same half-life of 193 s. What is the order of the reaction? What is the value and unit of the rate constant for this reaction?


The reaction exhibits a first-order dependence, as evidenced by its reaction order of 1. The magnitude and unit of the rate constant for this reaction are 5.92*10^-3 s^-1. In first-order reactions, the rate of reaction is contingent solely on the concentration of one reactant. Moreover, when the half life of a reaction does not vary with changes in concentration, it is reasonable to conclude that the reaction is first-order. Given: Half life = 117 s. Using the relationship between the rate constant and the half-life of a first-order reaction, the rate constant (k) can be calculated using k = ln 2 / half life, which returns a value of 0.693/(117) s^-1 or 5.92*10^-3 s^-1. Additional information concerning reaction rates can be found through the following link: brainly.com/question/24795637 #SPJ4.