Question

A specific reaction is known to have a first-order rate expression. If k = 1.52×10^-2/min, what is the half-life, in minutes, of this reaction? A. 91.2, B. 66.7, C. 33.3, or D. 45.6

Answer 1

For a first-order reaction with a rate constant of 1.52×10-2/min, the half-life is calculated using the formula t₁/₂ = 0.693/k, which results in D. 45.6 minutes.

Step-by-step explanation:

The half-life of a first-order reaction is independent of the initial concentration and can be determined using the formula t₁/₂ = 0.693/k, where k is the rate constant of the reaction. Given a rate constant k = 1.52×10-2/min for the first-order reaction, we can calculate the half-life as follows:

t₁/₂ = 0.693/(1.52×10-2/min) = 45.6 minutes.

Therefore, the correct answer is D. 45.6 minutes.