Iodine clock reaction. How do I find k, m and n? update: Reaction Mixture Final
ID: 1035630 • Letter: I
Question
Iodine clock reaction. How do I find k, m and n?
update:
Reaction Mixture
Final Concentration of I-
Final Concentration of S2O32-
Final Concentration of S2O82-
Final Concentration of I2
Average Time
Initial Rate M/s
1
0.04
0.0012
0.04
0.0006
50.93
1.17809E-05
2
0.08
0.0012
0.04
0.0006
20.4733333
2.93064E-05
3
0.04
0.0012
0.08
0.0006
57.08
1.05116E-05
Reaction Mixture
Final Concentration of I-
Final Concentration of S2O32-
Final Concentration of S2O82-
Final Concentration of I2
Average Time
Initial Rate M/s
1
0.04
0.0012
0.04
0.0006
50.93
1.17809E-05
2
0.08
0.0012
0.04
0.0006
20.4733333
2.93064E-05
3
0.04
0.0012
0.08
0.0006
57.08
1.05116E-05
FILE HOME INSERT PAGE LAYOUT FORMULAS DATA REVIEWVIEW E12 S203 M Time in seconds Initial rate of s203 initial rate of 12 2 |Run 1: 0.00096 0.000964 0.000964 Invalid data 0.000964 0.000964 0.000964 0.000964 0.000964 Invalid data 0.000964 Invalid data 72.47 29.39 1.33021E-05 3.28003E-05 6.65103E-06 1.64001E-05 Invalid data Invalid data 5 Run 2 24.24 17.16 20.02 57.08 3.9769E-05 5.61772E-05 4.81518E-05 1.68886E-05 1.98845E-0S 2.80886E-05 2.40759E-05 8.44429E-06 8 Run 3 9 10 Invalid data Invalid data Invalid data Invalid data 12 13 14 15 16 17 18 19 SheetlExplanation / Answer
Iodine clock reaction: 2 I? + S2O82? ? I2 + 2 SO42?
I2 + 2 S2O32? ? 2 I? + S4O62?
therefore rate of reaction can be written as: rate = k [ S2O82?]m [I?]n
substituing the values of these from the given table,
we can have 2 equations and 2 variables that can be easily solved,
we get,
m = 1 and n = 0
therefore overall reaction follows 1st order kinetic, hence rate constant k can be determined by
rate = k [ S2O82?]
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