Complete the lab report according to the requirements of LAB REPORT GRADING RUBRIC. I have attached an example for reference. I need to finish it by 1pm on February 11th, California time.need to complete (In this experiment you will confirm the validity of Newton’s 2nd Law by analyzing the motion of two objects (glider and a hanging mass) on a horizontal air track. First, you will calculate the theoretical acceleration by applying Newton’s 2nd Law (Fnet = MA), neglecting friction, to the glider and hanging mass. Next, you will calculate the experimental acceleration of the glider by applying the kinematic equations of motion as it moves between two markers (photogates) on the track. We will then compare the experimental acceleration to the theoretical acceleration: 1) Calculate the theoretical acceleration atheo of the system by applying Newton’s 2nd Law. 2) Calculate the experimental acceleration aexp of the system by two different methods using the kinematic equations of motion. 3) Compare aexp with atheo. .............)

The purpose of this assignment is to teach students how to better evaluate sources. By learning how to evaluate sources, students will better understand additional reasoning skills, such as induction, inference, deduction, and analysis. This assignment will appear at the beginning of this course to best prepare students for the upcoming QEP Assignment, in which evaluation is an important component. Students are encouraged to first review the included rubric to best understand the criteria in which they will be graded, and the benchmarks they should aim to achieve.       

Kinetics Activity Handout FormNote: You will need to use a spreadsheet program (excel), or other mathematical program (matlab, Mathcad, mathematica, R etc.) to complete this assignment. The blackboard site has links to a video introducing excel, along with excel spread sheets that contain the data for question 3.1) (4 pts) This form accompanies the online kinetics activity. Please use it to answer the following questions:Step-1a) Attach the printout of your kinetic trace and fill in the following data table: Volume of dye solution Concentration of bleach solution Volume of bleach solution b) What are the initial concentrations of [Yellow Dye] and [Bleach] for your experiment?undefinedStep-2undefined c) What is the value of the pseudo rate constant for your experiment?undefinedStep-3undefined d) Design an experiment to determine the order of the reaction with respect to [bleach]. Attach a printout of your kinetic trace from your experiment. Give the order with respect to [bleach] and explain how you determined this from the experiment. undefinedundefined Step-4undefinede) What is the proportionality constant, ε l, in Beer’s law, abs=ε l [dye]? Include units in your answer. (Abs is unitless and [dye] is in mol/L or M.)undefinedf) Calculate the rate constant (k) for the reaction of Yellow 6 with bleach to 2 significant figures, assuming the concentration of [dye] and [bleach] are in M.Write the rate law for the reaction (including both the numerical value of k, and the order of the reaction with respect to [dye] and [bleach]).undefined undefinedundefined3) (4 pts total) The following shows results from experiments similar to those of the online tutorial, but with different dyes and bleach. The reaction has 1:1 stoichiometry.undefineddye + bleach à colorless productsundefinedThe initial solutions have the following concentrationsundefinedBlue dye:3.20 x 10-5 MRed dye: 5.60 x 10-5 MBleach: 0.150 MundefinedThe absorbance was measured at various dye concentrations and the results are summarized below. undefined [blue dye] abs [red dye] abs 0 0 0 0 3.20E-06 0.08 5.60E-06 0.085 6.40E-06 0.16 1.12E-05 0.17 9.60E-06 0.24 1.68E-05 0.255 1.28E-05 0.32 2.24E-05 0.34 1.60E-05 0.4 2.80E-05 0.425 1.92E-05 0.48 3.36E-05 0.51 2.24E-05 0.56 3.92E-05 0.595 2.56E-05 0.64 4.48E-05 0.68 2.88E-05 0.72 5.04E-05 0.765 3.20E-05 0.8 5.60E-05 0.85 undefinedYou will need to make Beer’s Law Plots for both the blue dye and Red dye to be able to convert the absorbance measured to concentration of respective dye.undefinedundefinedExperiments were then performed by mixing the following volumes of dye and bleach solutions and monitoring absorbance versus time. undefinedExperiment 1:blue dye: 9.50 mLbleach: 0.500 mLundefinedExperiment 2:blue dye: 9.00 mLbleach: 1.00 mLundefinedExperiment 3:red dye: 9.50 mLbleach: 0.500 mLundefinedExperiment 4:red dye: 9.00 mLbleach: 1.00 mLundefinedThe results of the experiments (time and absorbance of dye used) are below:undefined time exp 1 exp 2 exp 3 exp 4 0 0.76 0.72 0.8075 0.765 10 0.638303 0.528549 0.746774 0.559157 20 0.550246 0.41766 0.69062 0.408725 30 0.483564 0.345287 0.638696 0.298778 40 0.431313 0.294318 0.590679 0.218413 50 0.389263 0.256477 0.546277 0.159668 60 0.35469 0.227266 0.505217 0.116726 70 0.325763 0.204035 0.467245 0.085333 80 0.301201 0.185116 0.43213 0.062384 90 0.280086 0.169411 0.399657 0.045607 100 0.26174 0.156164 0.369625 0.033342 110 0.24565 0.144839 0.341852 0.024376 120 0.231426 0.135047 0.316167 0.017821 130 0.218759 0.126496 0.292413 0.013028 140 0.207408 0.118964 0.270445 0.009525 150 0.197177 0.112279 0.250128 0.006963 160 0.187909 0.106306 0.231338 0.005091 170 0.179473 0.100936 0.21396 0.003722 180 0.171762 0.096083 0.197888 0.002721 190 0.164687 0.091676 0.183024 0.001989 200 0.158172 0.087655 0.169277 0.001454 undefineda) (2 pts) Determine the rate law of the reaction (including the rate constant, and order with respect to [dye] and [bleach]):undefinedblue dye + bleach à colorless productsundefinedPlease describe your approach, including any calculations or plots used for the analysis.undefinedundefinedb) (2 pts) Determine the rate law of the reaction (including the rate constant, and order with respect to [dye] and [bleach]):undefinedred dye + bleach à colorless productsundefinedPlease describe your approach, including any calculations or plots used for the analysis.