Determination of the equilibrium constant for the iodine + iodide →triiodide reaction as a function of concentration. Calculate the concentrations of iodine ([I2 ]0) and iodide ([I-]0) that would result from the dilutions if a reaction did not occur. Using the absorption measurement for triiodide (A) and its extinction coefficient, calculate the triiodide concentration ([I3-]) that results from achievement of equilibrium, them calculate the final concentrations of iodine ([I2]) and iodide ([I-]) bysubtraction. Finally, calculate the value of the equilibrium constant (Keq).
|
v (I2)
|
V (KI)
|
V (h2o)
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[I2] M
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[I-] M
|
A
|
T (celcius)
|
I3 M
|
I2 M
|
I- M
|
|
2
|
1
|
1
|
|
|
.505
|
23.3
|
|
|
|
|
1
|
2
|
1
|
|
|
.321
|
23.5
|
|
|
|
|
1
|
1
|
2
|
|
|
.249
|
22.2
|
|
|
|
|
3
|
1
|
0
|
|
|
.682
|
22.4
|
|
|
|
|
1
|
3
|
0
|
|
|
.322
|
21.9
|
|
|
|