The decomposition reaction of A to B is a second-order reaction with a half-life of 1.40x10$^2$ seconds: A $\rightarrow$ 2B If the initial concentration of A is 0.129 M, how many minutes will it take for the concentration of A to decrease by 89.9%?

          The decomposition reaction of A to B is a second-order reaction with a half-life of 1.40x10$^2$ seconds:
A $\rightarrow$ 2B
If the initial concentration of A is 0.129 M, how many minutes will it take for the concentration of A to decrease by 89.9%?

The decomposition reaction of A to B is a second-order reaction with a half-life of 1.40x10^2 seconds:
A → 2B
If the initial concentration of A is 0.129 M, how many minutes will it take for the concentration of A to decrease by 89.9%?

Added by Catalina R.

Calculus: Early Transcendentals

James Stewart 8th Edition

Instant Answer

Solved by Expert Adi S

06/29/2023

Step 1

The half-life of a second-order reaction can be related to the rate constant (k) using the equation: t1/2 = 1 / (k * [A]0) where t1/2 is the half-life, [A]0 is the initial concentration of A, and k is the rate constant. Given t1/2 = 1.40x10^2 seconds and [A]0 = Show more…

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(Incorrect)\nThe decomposition reaction of A to B is a second-order reaction with a half-life of 1.40\\times 10^(2) seconds:\nA->2B\nIf the initial concentration of A is 0.129M, how many minutes will it take for the concentration of A to decrease by 89.9% ? (Incorrect) The decomposition reaction of A to B is a second-order reaction with a half-life of 1.40x102 seconds: A-2B If the initial concentration of A is 0.129 M, how many minutes will it take for the concentration of A to decrease by 89.9%