Reaction kinetics

Experiment Objectives:

  • investigate the effect of reactant concentration on the rate of the iodide-persulphate reaction: S2O8-2 + 2I → I2 + 2SO4-2
  • experimentally derive the rate law for the reaction and determine the order of the reaction with respect to S2O8-2 and I
  • determine the reaction rate and rate constant under experimental conditions
  • observe the effect of varying the ionic strength of the reaction mixture on the rate and rate constant for this reaction

Experiment Results and Observations:

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Trial # Elapsed Time
1  
2  
3  
4  
5  
6  
7  

           

 

 

 

 

 

 

 

 

  Other physical observations:


 

Calculations and Results:

Show the calculations for trial #1 for the following: (Do not show calculations from any other trial; simply record all other values in the results table with appropriate units and significant digits)

Concentration of S2O8-2

 

 

 

 

 

Concentration of I

 

 

 

 

 

Concentration of S2O3-2

 

 

 

 

 

-DS2O8-2

 

 

 

 

 

 

Determining the exponents m and n:

Prepare the following two plots and attach them as the next two pages of your report.  Refer to Appendix B:  How to plot experimental data, when preparing these plots.

  1. a) Plot -log Dt versus log [S2O8-2] using the values from runs 1, 2, and 3
  2. b) Plot -log Dt versus log [I] for runs 1, 4, and 5.

On each graph, show a calculation for the slope.  If you have used a graphing program to solve for the slope, indicate the equation of the line and clearly identify the slope in this equation.  From the slopes of these two graphs determine the exponents m and n for the rate law.

Show your calculations from trial #1 for the following: (Do not show calculations from any other trial; simply record all other values in the results table with appropriate units and significant digits)

Rate

 

 

 

 

Rate Constant

 

 

 

 

Ionic Strength

 

 

 

 

Results Table:

Trial # [S2O8-2] [I] [S2O3-2] -DS2O8-2 Dt Rate k, Rate Constant Ionic Strength
1

 

               
2

 

               
3

 

               
4

 

               
5

 

               
6

 

               
7

 

               

 

Calculate the average rate constant for this reaction using data from trials 1 to 5.

 

 

 

 

 

 

Why are the rate constant values from trials 6 and 7 not used when calculating the average rate constant?

 

 

 

 

 

 

 

In one or two words, indicate the effect on the rate of this reaction if:

  1. a) The S2O3-2 concentration was halved, keeping all other factors the same?

 

  1. b) The S2O8-2 concentration was doubled, keeping all other factors the same?

 

  1. c) The temperature of the solution was decreased?

 

 

In one or two words, indicate the effect on the rate constant of this reaction if:

  1. a) The S2O3-2 concentration was halved, keeping all other factors the same?

 

  1. b) The I concentration was doubled, keeping all other factors the same?

 

  1. c) The ionic strength of the solution was increased?

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Conclusion:

Write a formal lab report conclusion for this experiment and attach it to these report sheets.  Refer to Appendix A for information on writing formal lab reports.  This conclusion should be no longer than one page.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

References:

If you use any resources in preparing this report, you must provide reference information for them here. Follow the guidelines in LEARN – Content – Lab reports.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Attachments to your report:

Attach the following 3 items in the space below (use an additional page if needed).  You may cut and paste, (a snipping tool is nice for this) or use an image or scan.

  • The randomized Data Set that you were provided to write this report
  • Your own Data Sheet with your written observations
  • Pre-lab questions

 

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