Question

a reactant decomposes with a half-life of 103 s when its initial concentration is 0.336 m. when the initial concentration is 0.573 m, this same reactant decomposes with the same half-life of 103 s. what is the order of the reaction? 2 1 0 what is the value and unit of the rate constant for this reaction?

Answer 1

The reaction is second order and the rate constant is approximately 9.7 × 10-6 M-2 s-1.

Step-by-step explanation:

The half-life of a reaction is the time required for one-half of a given amount of reactant to be consumed. In this case, the reaction is second order because the half-life is the same for different initial concentrations of the reactant. The rate constant for this reaction is not given in the question, but we can calculate it using the half-life equation for a second-order reaction:

Rate = k * [reactant]2

t1/2 = 1 / (k * [reactant])

Using the given half-life value of 103 s and the initial concentration of 0.336 M, we can solve for the rate constant:

k = 1 / (t1/2 * [reactant]) = 1 / (103 s * 0.336 M2)

k ≈ 9.7 × 10-6 M-2 s-1