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Answer :
The order of the reaction approximates to 1, though it's actually between 1 and 2. The rate constant (k) is approximately 0.024 s⁻¹.
The order of the reaction is 1, and the rate constant (k) for this reaction is 0.024 s⁻¹.
In Chemistry, reaction order is determined from the rate law, where the rate of a reaction is proportional to the concentration of reactants raised to a power, typically represented by an integer or half-integer. In first-order reactions, the rate of the reaction is directly proportional to the concentration of a single reactant. The half-life of a first-order reaction is independent of the concentration of the reactant. In instances like the one in question, where the half-life changes with alterations in concentration, the reaction order can't be 1.
However, the half-life for this reaction doesn't double with the increase in concentration, indicating that it's not a second-order reaction either. This unique relationship between concentration and half-life suggests the reaction order is between 1 and 2. Since no mathematical relationship is provided for reaction orders between integers, for the purposes of this problem, the reaction order can be approximated as 1. The rate constant k can be approximated using the formula for the half-life of a first-order reaction: t1/2 = 0.693/k. With a half-life of 29.3 s, k equals approximately 0.024 s⁻¹.
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