Determination of an Chemical Equilibrium Constant

Assignment Task

Use computer software ( or other program) to plot; include the graph with your lab report. Also using the software, perform a least squares, linear regression on the calibration data. This is most easily accomplished by adding a trendline (with Excel or other), determining the equation, Y = mx + b, for the 'line of best fit through the data points. Use the equation, not the graph itself, to find the equilibrium values of [FeSCN2'] 

Also, check if there appears to be an outlier among the points. If so, consider omitting the discrepant point(s) from the regression analysis. (In such a case, use two plots on the same graph: a plot of the suspect point(s), and a plot of the remaining points with a 'best fit' straight line through only them.) Indicate on your data sheet which points, if any, are being omitted. Details for plotting points and finding regression lines can be found on.

The assumption which was made, to allow calculation/ estimation of [FeSCN2*], means that the amount of SCN remaining in the solution is zero. This obviously cannot be so: equilibrium means that all these species will still exist, together, in solution. So, calculate the actual [SCN-] remaining in the middle solution - the - now that you have determined one using 2 mL of 0.00200 M KSCN - your best value of the equilibrium constant.

Is the assumption' a fair or reasonable one to make? Why, or why not? i.e. assume that the reaction goes all the way to the right, as Fe3+ SCN→ FeSCN2+, when the Fe3+ is in vast excess; then, SCN acts as the limiting reagent.

This Engineering has been solved by our PhD Experts at My Uni Paper.