Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 15.9 and 15.9 minutes respectively. If the rate constant is equal to 0.04358 and [A]0 = 11.98, calculate the [A] at t = 30.83 minutes.
Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 15.9 and 15.9 minutes respectively. If the rate constant is equal to 0.04358 and [A]0 = 11.98, calculate the [A] at t = 30.83 minutes.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the following reaction.
aA +bB →→ cC
whose first and second half-lives are 15.9 and 15.9 minutes respectively. If the rate constant is equal to 0.04358 and [A]0 = 11.98, calculate the [A] at t = 30.83 minutes.
Expert Solution
Step 1
Given data :
aA + bB ==> cC
first half life = 15.9 minutes
second half life = 15.9 minutes
rate constant = 0.04358
[A]0 = 11.98
t= 30.83 minutes
Identifying the order of reaction by using half life and rate constant relation :
rate constant = 0.693 / half life
if the rate constant from half life comes same as the given rate constant , the it is a first order reaction .
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