Determine the equilibrium constant Kc for the chemical reaction:
Fe3+(aq) + SCN-(aq) ß à FeSCN2+(aq)
|0.0020M Fe(NO3)3 (ml)||0.0020M KSCN (ml)||H2O (ml)|
(1) Calibrate the colorimeter.
(2) Prepare five test tubes with the designated solutions:
(3) Measure each solution using the colorimeter and computer software.
(4) Record an observation of the solution temperature.
(5) Calculate the average equilibrium constant for the reaction being studied, using the 5th test as the standard solution.
|Average Temperature: 23.5 C|
1. [Fe3+]i and [SCN-]i @ Trial 1
[Fe3+]i= 0.0020M Fe(NO3)3 x (5ml/10ml) = 0.001M, [SCN-]i = 0.0020M KSCN x (2ml/10ml) = 0.0004M
[FeSCN2+]std = 0.0020M x (2ml/20ml) = 0.0002M
3. [FeSCN2+]eq @ Trial 1
[FeSCN2+]eq= (Aeq/Astd) x [FeSCN2+]std = [(0.032/0.107) x 0.0002M=5.98×10-5M
4. [Fe3+]eq and [SCN-]eq @ Trial 1
[Fe3+]eq= 0.001 – (5.98×10-5) = 9.4 x 10-4M , [SCN-]eq = 0.0004 – (5.98×10-5) = 3.4 X 1O-4M
5. KC @ Trial 1 (23.5 degrees C)
Kc= [FeSCN2+]eq / [Fe3+]eq [SCN-]eq = (5.98×10-5)/(9.4 x 10-4)( 3.4 X 1O-4) = 187.0
6. Average Kc
Kc(avg) = ∑(Kc(trials 1->n))/ (n) = (187+97.86+118.79+128.81) / 4 = 133.1
In this experiment, the chemical reaction Fe3+(aq) + SCN-(aq) ß à FeSCN2+(aq) was studied to determine the equilibrium constant, Kc. To determine this value, the absorptivity of several solutions were recorded using a colorimeter. Inclusion of a standard solution allowed for equilibrium calculations of the reactant and product concentrations. Experimentally, the average constant Kc was calculated at (133.1). Linear analysis of the Kc range has revealed flaws in the first trial. The source of this error is probably due to Ryan’s inaccurate calibration of the colorimeter or poor handling of the solution.