em1.pngchem3.pngPart 3: Q9 Average absorbanceFlask 8Flask 9Flask 10Flask 11Part 3: Q9Flask 8Flask 9Flask 10Flask 11Part 3: Q10Flask 8Flask 9Flask 10Flask 11QPart 30.146[Fe] -0.002mol/L0.166volume 5.00mL0.2150.294[FESCN mol/L)✪4.59* 105.18*10*6.64 x 109.08*10*[Fe(mol/L)5.00 x 105.00*10*Y=3362x -0.0083 R¹ 0.99935.00 x 105.00*10*(Amounts of flask 8 (9 - 11's values are in the spreadsheet)1:1 Ratio so,Molarity of Fe(NO3))3 = 0.2MVolume of Fe(NO3))3 = 5.00mL71%Moles of Fe³= Molarity x volume(L)Moles of Fe = 0.2M × 0.005L = 1× 10-³mole68%[SCN ](mol/4 x 10-45 x 10-47*10*1*10*الخاchem2.pngConcentration of Fe³9,X =mole of Fe³1x10³ moleVolume0.0054Ⓒ8, Average absorbance for solution 8 (same for 9 - 11)Average absorbance for flask 8 = sum of all absorbances / number of readings(0.145 +0.147 +0.148)3Using equationof calibration curve's line(slope) of best fit, the average absorbances of theunknown concentrations to determine [FeSCN-]at equilibrium in solution 8:quation of line Y=3362x-0.0083For 8 with an average absorbance of 0.146(0.146 +0.0083)33620.146 = 3362X - 0.0083= 0.14610, [Fe] =25mlFe³ x 0.002mol/l-1100ml= 4.59 x 10-582%0.002M= 5.00 x 10-*mol/l-111. Place the results from calculations 9 and 10 into individual ICE tables. Calculate the equilibrium concentration ofFe³+ and SCN-in solutions 8 to 11.12. a) Calculate K, for each solution using the results of calculations 9 and 11. Calculate the average value of Kb) One published value of Ke for the equilibrium system under consideration is 146 at room temperature (Journalof Chemical Education, 75. pp 90). Determine a percent error for your average calculated value of K, based on thisliterature value.W6.png7 (blank)891011EQTABLE 2-COMPOSITION OF SOLUTIONS REQUIRED FOR CALCULATION OF EQUILIBRIUM CONSTANTVolume of 0.002 mol L-1 Volume of 0.002 mol L-1Flask #Fe(NO3)³(aq) / ml.KSCN(aq) / ml5.png25.0025.0025.0025.0025.00Ⓒ71%K₂0.0020.0025.00Ensure your Thermo Scientific Spectronic 200 spectrophotometer is powered on so that it is warmed up by thetime you use it later in the procedure.Pipette 5.00 mL of 0.2 mol L-4 Fe(NO3)³(aq) into a clean 500-mL volumetric flask. Fill the flask carefully to thecalibration mark with 1.0 mol L-¹ HNO3(aq). stopper it, and mix well by inversion (25 times). Pour about 175 mLof the solution you just prepared into a clean, dry 250-mL beaker. The concentration of Fe(NO3):(aq) in thissolution is approximately 0.002 mol L-4,Pipette the required volumes of 0.002 mol L-¹ Fe(NO3)3(aq) and then 0.002 mol L-4 KSCN(aq) into five clean,labelled 100-mL volumetric flasks. Before using the 25-mL pipette to deliver KSCN(aq) solution, remember to rinseit with this solution three times to remove any traces of Fe(NO3)(aq) that might be in it.Fill the flasks precisely to the calibration marks with deionized water. Remove any water droplets above the markswith a Kimwipe. Stopper the flask and mix each thoroughly by inverting it 25 times.Measure the absorbance of the solutions in flasks 8 through 11 as outlined in part 3 of the procedure.[F+SCN3[FON35.0050.00Fe (aq) + SCN- (aq) FeSCN²(aq)The equilibrium constant K, is a ratio of the product of the concentrations of the products to that of thereactants, with the concentrations raised to the power of their stoichiometric coefficients. So, for the reaction underconsideration61%In Part 1. solutions will be prepared with known concentrations of FeSCN³, a coloured species that can absorblight of a particular wavelength. The portion of incident light absorbed - called the absorbance - can be determinedusing an instrument called a spectrophotometer. The absorbance of the solutions will be plotted against [FeSCN³].resulting in a graph known as a calibration curve (even though the data is linear). By performing a linear regressionanalysis, it can be determined if the data conforms to Beer's Law. This law is used in spectroscopy to determineconcentrations of species in solution. It can be expressed asA = tbcwhere A is the absorbance. e is the molar absorptivity of the absorbing species. b is the length of solution through whichthe light passes (also called the path length), and c is the concentration of the absorbing species.In Part 2, the absorbance of solutions with unknown concentrations of FeSCN2 will be measured. Using thesemeasurements and the equation of the calibration curve line, the equilibrium concentration of FeSCN²(aq) in eachsolution can be determined. ICE tables are then used to find the equilibrium concentrations of all species present inEquation (2) and the equilibrium constant for Reaction (1) will be determined.

Given: [FeSCN+2] (mol/L) Flask 8 4.59×10-5 Flask 9 5.18×10-5 Flask 10 6.64×10-5 Flask…

Part 3: 09 Average absorbance prorhande Flask 8 Flask 9 Flask 10 Flask 11 Part 3: Q Flask 8 Flask 9 Flask 10 Flask Part 3: Q 10 Flask 8 Flask 9 Flask 10 Flask 11 Part 3 0.146 [Fe] -0.002mol/L 0.166 volume 5.00m 0.215 0.294 [FESCNmol/L) 4.59*10* 5.18*10* ✪ 6.6410 9.08*10 [Femol/L) 5.00*10* 5.00-10 Y=3362x-0.0083 R² = 0.9993 5.00-10 5.00*10* k 8 (9 – 11's values are in the spreadsheet) Ratio so 71% Molarity of Fe(NO3))3 = 0.2M Volume of Fe(NO3))3 = 5.00mL Moles of Fe = Molarity x volume(L) Fe 0.2M x 0.005L 1x 10 mole [SCN (mol/ 4 x 10-4 5x10-1 7*10* 1*10* Concentration of Fe³ =? mole of F Volume 8. Average absorbance for solution 8 (same for 9 - 11) Average absorbance for flask 8 = sum of all absorbances / number of readings 9. X = (0.145+0.147 +0.148) 1×10=0.002M 3 Using equation of calibration curve's line(slope) of best fit, the average absorbances of the unknown concentrations to determine (FeSCN-Jat equilibrium in solution 8: quation of line Y=3362x -0.0083 For 8 with an average absorbance of 0.146 0.146 = 3362X-0.0083 (0.146 +0.0083) 3362 0.0054 = 0.146 10, [Fe³] =25mlFe³x0.002mol/l-1 100ml -=4.59 x 10- -= 5.00 x 10-*mol/l-¹ 11. Place the results from calculations 9 and 10 into individual ICE tables. Calculate the equilibrium concentration of Feland SCN-in solutions 8 to 11. 12. a) Calculate K, for each solution using the results of calculations 9 and 11. Calculate the average value of K b) One published value of K, for the equilibrium system under consideration is 146 at room temperature (Journal of Chemical Education. 75. pp 90). Determine a percent error for your average calculated value of K, based on this literature value. TABLE 2-COMPOSITION OF SOLUTIONS REQUIRED FOR CALCULATION OF EQUILIBRIUM CONSTANT Volume of 0.002 mol L-¹ Volume of 0.002 mol L Flask # Fe(NO3)2(aq) / ml. KSCN[an) / ml W 7 (blank) 8 9 10 11 25.00 25.00 5.png 25.00 25.00 25.00 Ensure your Thermo Scientific Spectronic 200 spectrophotometer is powered on so that it is warmed up by the time you use it later in the procedure. Pipette 5.00 mL of 0.2 mol L4 Fe(NO)(aq) into a clean 500-mL volumetric flask. Fill the flask carefully to the calibration mark with 1.0 mol L-¹ HNO3(aq). stopper it, and mix well by inversion (25 times). Pour about 175 mL of the solution you just prepared into a clean, dry 250-mL beaker. The concentration of Fe(NO):(aq) in this solution is approximately 0.002 mol LA, Pipette the required volumes of 0.002 mol L4 Fe(NO3)(aq) and then 0.002 mol L4 KSCN(aq) into five clean. labelled 100-mL volumetric flasks. Before using the 25-mL pipette to deliver KSCN(aq) solution, remember to rinse it with this solution three times to remove any traces of Fe(NO1)(aq) that might be in it. Fill the flasks precisely to the calibration marks with deionized water. Remove any water droplets above the marks with a Kimwipe. Stopper the flask and mix each thoroughly by inverting it 25 times. Measure the absorbance of the solutions in flasks 8 through 11 as outlined in part 3 of the procedure. ... Q 0.00 20.00 25.00 35.00 KAN 50.00 61% Fe²(aq) + SCN- (aq) un FeSCN²(aq) The equilibrium constant K, is a ratio of the product of the concentrations of the products to that of the reactants, with the concentrations raised to the power of their stoichiometric coefficients. So, for the reaction under consideration In Part 1. solutions will be prepared with known concentrations of FeSCN³, a coloured species that can absorb light of a particular wavelength. The portion of incident light absorbed-called the absorbance-can be determined using an instrument called a spectrophotometer. The absorbance of the solutions will be plotted against [FeSCN³ resulting in a graph known as a calibration curve (even though the data is linear). By performing a linear regression analysis, it can be determined if the data conforms to Beer's Law. This law is used in spectroscopy to determine concentrations of species in solution. It can be expressed as A = ebe where A is the absorbance. e is the molar absorptivity of the absorbing species. b is the length of solution through which the light passes (also called the path length), and c is the concentration of the absorbing species. In Part 2. the absorbance of solutions with unknown concentrations of FeSCN will be measured. Using these measurements and the equation of the calibration curve line, the equilibrium concentration of FeSCN³(aq) in each solution can be determined. ICE tables are then used to find the equilibrium concentrations of all species present in Equation (2) and the equilibrium constant for Reaction (1) will be determined.