Question

Consider the following first-order reaction: A → B. The concentration of A at the start of the reaction is 4.15 M and after 4.99 s is 3.54 M. (a) Using the integrated rate law for a first-order reaction, calculate the value of the rate constant. s^(-1) (b) Calculate the half-life of the reaction. s

Name: consider the following first order reaction a b the concentration of a at the start of the reaction is 415 m and after 499 s is 354 m a using the integrated rate law for a first order reacti 82708
Uploaded: 2023-03-02T01:30:28-08:00
Duration: 3 min 31 s
Channel: Syon Schlecht
Description: consider the following first order reaction a b the concentration of a at the start of the reaction is 415 m and after 499 s is 354 m a using the integrated rate law for a first order reacti 82708

          Consider the following first-order reaction: A → B.
The concentration of A at the start of the reaction is 4.15 M and after 4.99 s is 3.54 M.
(a) Using the integrated rate law for a first-order reaction, calculate the value of the rate constant. s^(-1)
(b) Calculate the half-life of the reaction. s

Added by Aurora P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Syon Schlecht

03/02/2023

Step 1

We are given that $[A]_0 = 4.15\,\text{M}$, $[A] = 3.54\,\text{M}$, and $t = 4.99\,\text{s}$. We can plug these values into the integrated rate law equation and solve for $k$: $$\ln\frac{4.15}{3.54} = k(4.99)$$ $$k = \frac{\ln\frac{4.15}{3.54}}{4.99}$$ Now, we Show more…

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Consider the following first-order reaction: A → B. The concentration of A at the start of the reaction is 4.15 M and after 4.99 s is 3.54 M. (a) Using the integrated rate law for a first-order reaction, calculate the value of the rate constant. s^(-1) (b) Calculate the half-life of the reaction. s