CHEM 1F92 Lecture Notes - Lecture 16: Rate Equation, Reaction Rate Constant
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The integrated rate laws for zero-, first-, and second-orderreaction may be arranged such that they resemble the equation for astraight 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 zero-order reaction was 6.00
The integrated rate laws for zero-, first-, and second-orderreaction may be arranged such that they resemble the equation for astraight 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 zero-order reaction was 6.00
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 |
Part A
The reactant concentration in a zero-order reaction was 5.00Ã10?2M after 175 s and 4.00Ã10?2M after 400 s . What is the rate constant for this reaction?
Part B
What was the initial reactant concentration for the reaction described in Part A?
Part C
The reactant concentration in a first-order reaction was 6.40Ã10?2M after 50.0 s and 4.60Ã10?3M after 60.0 s . What is the rate constant for this reaction?
Part D
The reactant concentration in a second-order reaction was 0.730 M after 210 s and 6.40Ã10?2M after 705 s . What is the rate constant for this reaction?