Part I: Preparation of a standard absorption curve for FeSCN+2
Standard | 0.20M Fe(NO3)3 | 0.0020 M KSCN | 0.100M HNO3 | [FeSCN+2] | Absorbance |
A
|
10.0 mL | 0.0 mL | 15.0 mL | 0 | 0 |
B
|
10.0 mL | 1.0 mL | 14.0 mL | 0.00008M | 0.312 |
C
|
10.0 mL | 1.5 mL | 13.5 mL | 0.00012M | 0.503 |
D
|
10.0 mL | 2.0 mL | 13.0 mL | 0.00016M | 0.725 |
E
|
10.0 mL | 2.5 mL | 12.5 mL | 0.0002M | 1.025 |
F
|
10.0 mL | 3.0 mL | 12.0 mL | 0.00024M | 1.045 |
EQUATION: y=0.2167x-0.1569 R2_=0.9711______
Part 2: Measuring Equilibrium
Test Solution | 0.0020 M Fe(NO3)3 | 0.0020 M
KSCN |
0.10 M
HNO3 |
Initial [Fe+3] | Initial [SCN–] | Absorbance | Equilibrium
[FeSCN+2]* |
I
|
5.0 mL | 0 | 5.0 mL | 0.0010M | 0 | 0 | 0M |
II
|
5.0 mL | 1.0 mL | 4.0 mL | 0.0010M | 0.00020M | 0.206 | 4.9×10^-5M |
III
|
5.0 mL | 2.0 mL | 3.0 mL | 0.0010M | 0.00040M | 0.348 | 7.9×10^-5M |
IV
|
5.0 mL | 3.0 mL | 2.0 mL | 0.0010M | 0.00060M | 0.558 | 1.2×10^-4M |
V
|
5.0 mL | 4.0 mL | 1.0 mL | 0.0010M | 0.00080M | 0.782 | 1.7×10^-4M |
VI
|
5.0 mL | 5.0 mL | 0.0 mL | 0.0010M | 0.0010M | 0.815 | 1.8×10^-4M |
* To be determined from the standard graph equation.
ANALYSIS:
- Use your graph equation to calculate the equilibrium concentrations of FeSCN+2.
- Prepare and ICE chart for each test solution (II – VI) and calculate the value of Keq for each of your 5 tests solutions.
SAMPLE ICE CHART
Test Solution
Keq =343.9 |
Fe3+ + SCN– ⇄ FeSCN2+ | ||
I
|
0.0010M | 0.00020M | 0 |
C
|
-x | -x | +x |
E
|
0.00095M | 0.00015M | 4.9×10^-5M |
SAMPLE ICE CHART
Test Solution
Keq =268.3 |
Fe3+ + SCN– ⇄ FeSCN2+ | ||
I
|
0.0010M | 0.00040M | 0 |
C
|
-x | -x | +x |
E
|
0.00092M | 0.00032M | 7.9×10^-5M |
SAMPLE ICE CHART
Test Solution
Keq =284.0 |
Fe3+ + SCN– ⇄ FeSCN2+ | ||
I
|
0.0010M | 0.00060M | 0 |
C
|
-x | -x | +x |
E
|
0.00088M | 0.00048M | 1.2×10^-4M |
SAMPLE ICE CHART
Test Solution
Keq =325.1 |
Fe3+ + SCN– ⇄ FeSCN2+ | ||
I
|
0.0010M | 0.00080M | 0 |
C
|
-x | -x | +x |
E
|
0.00083M | 0.00063M | 1.7×10^-4M |
SAMPLE ICE CHART
Test Solution
Keq =267.7 |
Fe3+ + SCN– ⇄ FeSCN2+ | ||
I
|
0.0010M | 0.0010M | 0 |
C
|
-x | -x | +x |
E
|
0.00082M | 0.00082M | 1.8×10^-4M |
CONCLUSION AND EVALUATION:
- Comment on your Keq values. Do your results convince you that Keqis a constant value regardless of the initial concentrations of the reactants? Why or why not?
Because the Keqequals the concentration of products divided by the concentration of the reactants. If we change the initial concentrations of the reactants, it changes the equilibrium concentration of the reactants. So it also changes the Keq.
- Calculate the average value of Keqfrom your five trials. The actual value of Keq for this reaction at 25oC is reported as 280. Calculate (should you use all of your values?) the percent difference of your average value from the reported value:
% difference = (experimental value – reported value) x 100%
Reported value
Average value for Keq= (343.9+268.3+284.0+325.1+267.7)/5=297.8
1: % difference=100%(343.9-280.0)/280.0=22.9%
2: % difference=100%(268.3-280.0)/280.0=4.18%
3: % difference=100%(284.0-280.0)/280.0=1.43%
4: % difference=100%(325.1-280.0)/280.0=16.1%
5: % difference=100%(267.7-280.0)/280.0=4.39%
The graph for part one