CHEM 115 Lecture Notes - Lecture 6: 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.
1.) The reactant concentration in a zero-order reaction was 6.00Ã10â2M after 165 s and 3.50Ã10â2Mafter 385 s . What is the rate constant for this reaction?
2.)What was the initial reactant concentration for the reaction described in Part A?
3.)The reactant concentration in a first-order reaction was 6.70Ã10â2
M after 40.0 s and 2.50Ã10â3Mafter 95.0 s . What is the rate constant for this reaction?
4.)The reactant concentration in a second-order reaction was 0.850
M after 255 s and 3.40Ã10â2M after 860 s . What is the rate constant for this reaction?
Order | Integrated Rate Law | Graph | Slope |
0 | [A]=âkt+[A]0 | [A] vs. t | âk |
1 | ln[A]=âkt+ln[A]0 | ln[A] vs. t | âk |
2 | 1[A]= kt+1[A]0 | 1[A] vs. t | k |