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Report: Experiment M (Effect of Concentration on Reaction Rate) \& Experiment N (Effect of Temperature on Reaction Rate) Name: Bench \# Section: Date: Laboratory Instructor: Part I: Rate Law Determination For the calculations in Part luse the data from Experiment $M$, unless instructed otherwise 1. Using the molar absorptivity ( $?$, calculated in Question 2 of the Advance Study Assignment on page M-8) convert each of the absorbance values from the kinetic measurements to the corresponding concentration of crystal violet and then prepare plots of $[CV_{?}]$ versus $t_{,}ln[CV_{?}]$ versus $t$, and $1/[CV_{?}]$ versus $t$. Prepare these three graphs for one of your runs, preferably the run using the highest [ $OH_{?}]$. Include these three plots with your Lab Report. Note: You will likely have already constructed these plots before leaving the lab during Experiment $M$ and can simply submit them with this report. $(2.0)$ 2. Based on your plots in Question 1 , what is the order of the reaction with respect to crystal violet? Explain how you determined this. (1.0) 3. Explain how you can determine the pseudo rate constant $K$ for Run 1 from a graph you prepared in Q1 above. Plot the appropriate graphs for Runs 2 and 3 and write all three $k_{?}$ values to the table at the top of page $N?14$. Be sure to indicate units for $k_{?}$ and to express your $k_{?}$ values using an appropriate number of significant digits. (1.0) 4. Calculate the initial concentrations of $OH?(aq)$ for each kinetics run: these initial concentrations represent the concentrations of $OH_{?}$at the moment of mixing, before any reaction with $CV+$ has taken place. Place these values into the table on page $N?14(1.0)$
5. Using the ratio method described on pages M-5 and M-6, determine the partial order of the reaction with respect to the hydroxide ion. To do this, perform the calculation three times: compare Run 1 to Run 2, compare Run 1 to Run 3, and compare Run 2 to Run 3. Determine the average of your three results, and round it to the nearest integer. (1.0) 6. Calculate the value of $k$ for each run and add these values to the table at the top of this page and indicate the units for $k$. Show your calculations for Run 1 . Determine the average overall rate constant $k$. (1.0)
8. Explain why the reaction temperature was measured for each run in Experiment $M,(0.5)$ 9. Using the values from Run 1 of Experiment $M$, determine the value for $[OH]$ at $t=120s$. What percentage of the initial amount of hydroxide is consumed during the 120 seconds? Is this consistent with our treatment of the run as pseudo-first order? (Hint. What amount of [CV $_{?}]$ is consumed during this time?) (1.5)
10. If you performed another run in which $[OH_{?}]$; was identical to [ $CV_{?}]$, would a plot of $ln[CV_{?}]$ versus time reveal a straight-line relationship? Would any of the three types of integrated ratelaw plot reveal a linear relationship? Explain your answers. (1.0) Part II: Activation Energy Calculations For the calculations in Part II use the data from Experiment N, unless instructed otherwise 1. Show your calculation for the initial molarity of oH for the Experiment $N$ kinetics runs in the space below. Note: This refers to the concentration of the $OH$ at the point of mixing ( Le. before reaction: account for dilution!). (0.5) 2. Based on the order of reaction with respect to $CV$, as determined in Experiment $M$, prepare (for each of the four runs) the appropriate integrated rate law plot and determine $k_{?}$ and $k$ for each run. For best results, use only the data points from 60 s to 120 s inclusive for each run. Do not attach these plots to your lab report: simply report the experimental values for $k_{?}$ and $k$ in the above table, and include the corresponding temperature values from Observation Sheet N-11. (1.5)
Complete the following table relating the temperature to reaction rate. (1.0) 1. Plot $ln(k)$ vs. $1/T(K_{?1})$ using Google Sheets or some other computer spreadsheet software. Your graph should include a best-fit line from software-calculated linear regression analysis. Include the data from $ExpM$ Run 1 as a data point as well. Attach the plot to your lab report. (1.0) 2. In the space below, write the linear equation (of the form $y=mx+b$ ) for the best-fit line for the data plotted above. Be sure to include units, even if they are absent in the equation as it appears in your software. Clearly identify and label both the slope and the $y$-intercept portions of this equation. (1.0) 3. Using the value of the slope of the best fit line, calculate the activation energy $(E_{a})$ for the reaction of $CV_{?}$ and $OH:$ (1.5)
4. Using the value of the $y$-intercept of the best fit line for the graph, calculate the preexponential factor $(A)$ for the reaction of $CV_{?}$ and $OH:(1.0)$ 5. Calculate the value of $k$ that should be obtained from a run performed at $5_{?}C$ Show your calculations. (1.5)

Experiment M is a study of the effect of concentration on reaction rate. The goal of this experiment is to determine the rate law for the reaction of

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