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+by=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0[A]=−kt+[A]0 [A] vs. t[A] vs. t −k−k 1 ln[A]=−kt+ln[A]0ln[A]=−kt+ln[A]0 ln[A] vs. tln[A] vs. t −k−k 2 1[A]= kt+1[A]01[A]= kt+1[A]0 1[A] vs. t1[A] vs. t kk Part C) The reactant concentration in a first-order reaction was 5.50×10−2 M after 20.0 ss and 1.00×10−3 M after 90.0 s. W
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+by=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0[A]=−kt+[A]0 [A] vs. t[A] vs. t −k−k 1 ln[A]=−kt+ln[A]0ln[A]=−kt+ln[A]0 ln[A] vs. tln[A] vs. t −k−k 2 1[A]= kt+1[A]01[A]= kt+1[A]0 1[A] vs. t1[A] vs. t kk Part C) The reactant concentration in a first-order reaction was 5.50×10−2 M after 20.0 ss and 1.00×10−3 M after 90.0 s. W
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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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+by=mx+b.
| Order | Integrated Rate Law | Graph | Slope |
| 0 | [A]=−kt+[A]0[A]=−kt+[A]0 | [A] vs. t[A] vs. t | −k−k |
| 1 | ln[A]=−kt+ln[A]0ln[A]=−kt+ln[A]0 | ln[A] vs. tln[A] vs. t | −k−k |
| 2 | 1[A]= kt+1[A]01[A]= kt+1[A]0 | 1[A] vs. t1[A] vs. t | kk |
Part C)
The reactant concentration in a first-order reaction was 5.50×10−2 M after 20.0 ss and 1.00×10−3 M after 90.0 s. What is the rate constant for this reaction?
Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
Part D)
The reactant concentration in a second-order reaction was 0.460 M after 150 s and 2.90×10−2 M after 705 s. What is the rate constant for this reaction?
Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
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