Find the best answers to your questions with the help of IDNLearn.com's knowledgeable users. Our platform provides detailed and accurate responses from experts, helping you navigate any topic with confidence.

Hypochlorous acid decays in the presence of ultraviolet radiation. Assume that degradation occurs accord- ing to first-order kinetics and the rate of degradation was measured to be 0.12 day−1 (at a particular sun- light intensity and temperature). Given this, how long does it take for the concentration of hypochlorous acid to reach nondetectable levels (0.05 mg · L−1) if the initial concentration were 3.65 mg · L−1?

Sagot :

Answer:

35.75 days

Explanation:

From the given information:

For first-order kinetics, the rate law can be expressed as:

[tex]\mathsf{In \dfrac{C}{C_o} = -kt}[/tex]

Given that:

the rate degradation constant = 0.12 / day

current concentration C = 0.05 mg/L

initial concentration C₀ = 3.65 mg/L

[tex]\mathsf{In( \dfrac{0.05}{3.65})= -(0.12) t}[/tex]

㏑(0.01369863014) = -(0.12) t

-4.29 = -(0.12)

t = -4.29/-0.12

t = 35.75 days