Final answer:
The half-life of a zero-order reaction depends on the rate constant and initial concentration. For a reaction with an initial concentration of 0.834 M and a rate constant of 5.42 × 10⁻² M/s, the half-life is calculated as 7.69 seconds.
Step-by-step explanation:
The half-life of a zero-order reaction is the time required for the reactant concentration to decrease to one-half its initial value. In a zero-order reaction, this half-life depends on both the rate constant and the initial concentration of the reactant. The equation for the half-life of a zero-order reaction can be derived from the integrated zero-order rate law, which is [A] = -kt + [A]o. By setting [A] to one-half of [A]o, we can solve for the half-life.In this case, the initial concentration ([A]o) is 0.834 M and the rate constant (k) is 5.42 × 10⁻² M/s. The equation for the half-life (t1/2) of a zero-order reaction is given by t1/2 = [A]o / (2k). Plugging in the values, we get: t1/2 = 0.834 M / (2 × 5.42 × 10⁻² M/s)
After simplifying, the half-life of the reaction can be found. Thus, for a zero-order reaction with these specified conditions, the half-life is calculated to be 7.69 seconds.