A simple reaction follows first order kinetics. Complete the following table;

[Reactant]

0.600 M

0.400 M

0.300 M

0.250 M

Q1

Time (sec)

0

Q2

137

Q3

274

 

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Laboratory Section:

1. Determine the concentration of the reactant after 274 seconds.

2. How long does it take for the concentration of the reactant to fall to 0.400 M?

3. How long does it take for the concentration of the reactant to fall to 0.250 M?

When the first order integrate rate law is written in the following form;

ln[A]t = -kt + ln[A]o

The equation has the form of the equation for a straight line.

4. If the data in the table at the top of the page were plotted according to the equation,ln[A]t = -kt + ln[A]o, what would would be plotted on the y-axis and what would be plotted on the x-axis?

5. What does the slope of the line tell us and what is the y-intercept?

6. For a simple reaction that follows second order kinetics when the initial concentration is 0.0300 M the time required for the concentration to fall to 0.0150 m is 28 seconds. How long will it take for the concentration to fall to 0.0125 M? to 0.00625M?

7. Is there anything about the reaction or the questions that you feel you do not understand? List your concerns/questions.