1. The following data were obtained for the hypothetical reaction A + B → C + D
Experiment
[A] M
[B] M
Initial Rate (M/s)
1
0.100
0.0500
0.00313
2
0.300
0.100
0.0375
3
0.300
0.200
0.150
4
0.200
0.0500
0.00625
a. What is the order of the reaction with respect to A and B?
b. Write the rate law for the reaction.
c. Calculate k for the reaction.
2. A group mixes the following solutions for two trials, intending to keep [H2O2] constant and double [KI].
Experiment
Volume of 0.88 M H2O2
Volume of 0.50 M KI
Total Volume
1
2.00 mL
2.00 mL
4.00 mL
2
2.00 mL
4.00 mL
6.00 mL
a. Why might this not work to compare the effect of doubling [KI] from trial 1 to trial 2?
b. What could they do differently?
3. Without using numerical data, briefly describe how you could use pressure data to determine the rate for the reaction your group will be studying.
4. What specific concentrations of H2O2 and KI do you plan to use for your different trials (you should make a list)? (Remember, as mentioned under Useful Equipment, Techniques, and Concepts, it is much easier if you maintain a constant total volume for all trials!).

1. Determine the rate law for the reaction. Show your work.
2. Calculate k for the reaction. Show your work. Report the average value of k and its standard deviation.
3. Describe any sources of experimental uncertainty from the experiment.

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