The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0 [A] vs. t −k 1 ln[A]=−kt+ln[A]0 ln[A] vs. t −k 2 1[A]= kt+1[A]0 1[A] vs. t k The reactant concentration in a first-order reaction was 5.50×10−2 M after 25.0 s and 1.30×10−3 M after 100 s . What is the rate constant for this reaction? The reactant concentration in a second-order reaction was 0.250 M after 260 s and 6.60×10−2 M after 845 s . What is the rate constant for this reaction?
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0 [A] vs. t −k 1 ln[A]=−kt+ln[A]0 ln[A] vs. t −k 2 1[A]= kt+1[A]0 1[A] vs. t k The reactant concentration in a first-order reaction was 5.50×10−2 M after 25.0 s and 1.30×10−3 M after 100 s . What is the rate constant for this reaction? The reactant concentration in a second-order reaction was 0.250 M after 260 s and 6.60×10−2 M after 845 s . What is the rate constant for this reaction?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 21PS: At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an...
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The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+b.
| Order | Integrated Rate Law | Graph | Slope |
| 0 | [A]=−kt+[A]0 | [A] vs. t | −k |
| 1 | ln[A]=−kt+ln[A]0 | ln[A] vs. t | −k |
| 2 | 1[A]= kt+1[A]0 | 1[A] vs. t | k |
The reactant concentration in a first-order reaction was 5.50×10−2 M after 25.0 s and 1.30×10−3 M after 100 s . What is the rate constant for this reaction?
The reactant concentration in a second-order reaction was 0.250 M after 260 s and 6.60×10−2 M after 845 s . What is the rate constant for this reaction?
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