Final answer:
The half-life for a first-order reaction with a rate constant of 6.2 × 10⁻⁴ s⁻ⁱ is approximately 111.77 seconds.
Step-by-step explanation:
The half-life of a first-order reaction can be determined by using the relationship between the half-life (t₁₂) and the rate constant, k, which is given by the equation t₁₂ = 0.693/k. Given that the rate constant k for the reaction is 6.2 × 10⁻⁴ s⁻ⁱ, we can substitute this value into the equation to find the half-life of the reaction.
By substituting the given value of k into the equation, we get: t₁₂ = 0.693/(6.2 × 10⁻⁴ s⁻ⁱ) = 1.1177 × 10² s, or approximately 111.77 seconds. Therefore, the half-life for this first-order reaction is roughly 111.77 seconds.