1. Rate Law and Activation Energy Methyl Blue
Determining the Rate Law using the Time Dependent Rate

2. The Reaction

3. The Reaction
Reaction takes about 30 s to a few minutes depending on the initial concentrations
Can use a continuous monitoring method
Because there is a color change we can use spectroscopy

4. The Reaction
In this experiment, the initial concentration of the hydroxide is at least 1000 times larger than the concentration of the MB
This means that
And

5. Figuring out x
To figure out the order with respect to the MB+ we will observe [MB+] vs t
To do this we use Beer’s Law
Plot At vs t, LN(At) vs t and 1/At vs t to see if the reaction is zeroth order, first order or second order wrt MB+
Absorbance
Constants

6. The Math Zeroth Order First Order
The slope of the linear curve will get you k’=k[OH-]oy to within a constant
Repeating the experiment at a second [OH-] will get you access to how slope depends on [OH-] and get y
Second Order

7. Figuring out x At LN(At) 1/At If straight x = 0 If straight x = 1
Which one gives a straight line?

8. Part A: Set Up Spectrometer*
First we need to Calibrate the Spectrometer by placing an empty cuvette in the cuvette holder (follow instructions on the first page of the spectroVis handout sheet)
Once Calibrated we need to record the absorption spectrum of Methyl Blue, by placing a cuvette with MB in it in the spectrometer and collecting absorbance vs wavelength
Find the wavelength λmax of maximal absorption make a note in you notebook and print the graph for each group member
Set up the spectrometer to record absorbance vs time at λmax (see page 3 on the handout)
* Follow procedures set out in the Vernier handout

9. Part B: Determining x the order of reaction with respect to the Methyl Blue
Transfer contents of beaker 2 into beaker 1
0.1 M NaOH
Fill Cuvette and transfer to spectrometer
record absorbance 3 mins
Beaker 1
Measure 10 mL
Methyl Blue
Beaker 2
Measure 10 mL
NaOH

10. Part B: Determining x the order of reaction with respect to the Methyl Blue
Follow instructions in the lab manual to plot A vs t, LN(A) vs t and 1/A vs t
Fit each graph to a linear fit and determine which gives the best straight line this will tell you if x = 0, x = 1 or x = 2
Record data in your notebook
Do 5 trials and use the average to determine k’ = k[OH]y

11. Part C: Determining y the order of reaction with respect to the hydroxide
Repeat part B with 0.5M NaOH
Measure the absorbance vs time and determine k’= k[OH]y
Repeat 5 times to improve your statistics
Following the method shown in the sample report by taking the ratio of k[OH]y for the 2 concentrations y can be determined

12. Part D: Determining Ea and A
We need to determine the rate constant at different temperatures
Each group needs to perform
2 runs at a temperatures below room temperature
2 runs at a temperatures above room temperature
2 runs at room temperature
Post of the board the temperature (oC) and the slope of the LN(A) vs t graph

13. Part D: Determining Ea and A
ignition tubes
hotplate
methyl blue
0.1 M NaOH
thermometer
place NaOH in one ignition tube and the MB in the other sit them in a beaker of warm water sitting on the hot plate allow them time to reach thermal equilibrium record Tbefore
Then pour the contents from one tube into the other, leaving it in the water bath, stir with the thermometer and transfer some of the mixture into the cuvette
Record A vs t for 20 seconds
Measure the temperature of the solution in the cuvette after Tafter

14. Calculating Ea and A
Using your 6 trials, calculate k, ln(k), T(K) and 1/T
Make an Arrhenius plot ln(k) vs. 1/T