1. 1/6 points Last Response | Show Details All Responses Notes This question will involve error analysis. In the following table, enter the values called for from your experimental results. Then calculate the percent error for the differences between the values you obtained for the solution of unknown concentration in Part A, and the results you obtained in Part B and Part C. The equation for percent error is: % difference = ((theoretical value - actual value) x 100%) / theoretical value. A percent difference can be positive or negative.Treat the concentration you measured in Part A as the theoretical value, the one you're trying to match. TABLE A. Error analysis for copper(II) sulfate solution preparations.Absorbance at620 nm, AU*% Differencefrom UnknownConcentrationof Cu2+, M% Differencefrom UnknownUnknown, Part A0.230[0.230]0.376 [0.376]Solution from solid0.509[0.509]54.8 [-121]0.829 [0.829]54.6 [-120]Solution from stock solution0.599[0.599]61.6 [-160]0.976 [0.976]61.5 [-160]*AU = absorbance unitsThe absorbances and concentrations will be counted correct, but will not receive points. They were accounted for in your lab report.Why would you expect the % differences for the absorbance to be similar to the % differences for the concentration in each part of the experiment? (_) (_) Because the errors are most likely from using volumetric glassware and it was used in all the measurements. (o) (o) Because the concetration is calculated from the absorbance, the errors should be the same for both. (_) (_) You would not expect them to be similar, it is just by chance that they are in this experiment. (_) (_) Because the errors are most likely from the spectrometer and it wasused in all the measurements.(_) (_) You would not expect them to be similar and they are not for this expermiment. 2. 3/3 points Last Response | Show Details All Responses Notes These questions relate to the spectrometer. a. If the spectrometer had been set to a different wavelength to measure absorbances (one where the copper would have absorbed more or less light), how would that have changed the results? (o) (o) The results would have been the same. (_) (_) If the absorbance had been lower, the calculated unknown concentration would have been higher. (_) (_) There is not enough information to determine how this would have changed the calculated unknown concentration. (_) (_) If the absorbance had been greater, the calculated unknown concentration would have been lower. (_) (_) If the absorbance had been lower, the calculated unknown concentration would have been lower. (_) (_) If the absorbance had been greater, the calculated unknown concentration would have been higher. b. In this experiment, you used a 1 cm pathlength cell for all measurements. Would you expect the results (concentration of the unknown) to be different if a 0.1 cm pathlength cell had been used for all the measurements? (o) (o) You would expect the calculated unknown concentration to be the same. (_) (_) There is not enough information to determine how this would have changed the calculated unknown concentration but it would not be the same. (_) (_) You would expect the calculated unknown concentration to be lower. (_) (_) You would expect the calculated unknown concentration to be higher. c. What would have happened if you had used a cell with a different pathlength for measuring the unknown than the calibration standards?(o) (o) There is not enough information to determine how this would have changed the calculated unknown concentration but it would not be the same. (_) (_) You would expect the calculated unknown concentration to be the same. (_) (_) You would expect the calculated unknown concentration to be higher.(_) (_) You would expect the calculated unknown concentration to be lower. 3. 16/16 points Last Response | Show Details All Responses Notes Enter the values from your calibration curve's trendline below. y = 0.615 [0.615] x + -.000800 [-0.000800] Using your calibraion curve, please answer questions a - d. a. What is the concentration of a solution with an absorbance of 0.325?concentration = 0.530 [0.530] Mb. What absorbance would you expect from a solution of 0.1574 M concentration?absorbance = 0.096 [0.096]c. If a solution has an absorbance of 0.511 in a 1.00 cm pathlength cuvette, what would the absorbance be in a cuvette of 0.46 cm pathlength cell?absorbance = 0.235 [0.235]d. Calculate the molar absorptivity ( ) of Cu2+ at 620 nm given that the cuvettes used in lab had a pathlength of 1.00 cm.= 0.615 [0.615]