For the following questions (c and d), assume that the concentration of the hydroxide ion was initially 1.00 M, 3.00 M and 5.00 M (after mixing) for Runs #1, #2 and #3, respectively. c. Produce a plot of the pseudo-rate constants, Ln(k') vs. Ln [OH-], Calculation #7 on pg. 7. Determine the order of the hydroxide ion (Attach the relevant spreadsheet and plot). Order of OH-: (express as an integer) d. Using the intercept from the plot produced in 2c, determine the value for the rate constant, as described in Calculation #8 on pg. 7 k: 0.2647 Show your work here: K = e-3.6317 = 0.2647 3. Using the analysis in Question #2, determine the rate of reaction of chloromethane with the hydroxide ion at 61 °C, given initial concentrations of [CH3Cl] = [OH-] = 0.45 M?

For the following questions (c and d), assume that the concentration of the hydroxide ion was initially 1.00 M, 3.00 M and 5.00 M (after mixing) for Runs #1, #2 and #3, respectively. c. Produce a plot of the pseudo-rate constants, Ln(k') vs. Ln [OH-], Calculation #7 on pg. 7. Determine the order of the hydroxide ion (Attach the relevant spreadsheet and plot). Order of OH-: (express as an integer) d. Using the intercept from the plot produced in 2c, determine the value for the rate constant, as described in Calculation #8 on pg. 7 k: 0.2647 Show your work here: K = e-3.6317 = 0.2647 3. Using the analysis in Question #2, determine the rate of reaction of chloromethane with the hydroxide ion at 61 °C, given initial concentrations of [CH3Cl] = [OH-] = 0.45 M?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Q 11 please
Q 20 please
14. Consider the following energy diagram for a reaction. Calculate the activation energy Ea and the enthalpy of reaction AH. Is the reaction endothermic or exothermic? Energy (kJ/mol) 100 150 200 250 300 350 400 450 500 Reaction progress
What is the correct rate law for this reaction A(g) + 2B(g) -> 2C(g) + 2D(g)
Q 14 please
::((/(/(/(:(:)/
Consider the following reaction: H2O2(aq) H2O() + % 02(g) and the kinetics plots below to answer the questions to the right. Figure 1. Plot of [H,O;] vs time 1. 09 07 03 02 01 time (s) Figure 2. Plot of the natural logarithm of (H,O,] vs time 100 as -1 time (s) Infconcentration of H,0) concentration of H0, (mol L)
Question 19 of 28 How long will it take for the concentration of A to decrease from 0.500 M to 0.200 M in the first-order reaction A B? (k = 0.800 s1) %3D 1 3. 4 6. 7 8 9. +/- 11:45 P OType here to search 53°F Cloudy ^ 5/8/202 DOLL Esc F1 F2 F3 F4 第10 F5 F6 F7 F8 F9 F11 F12 PrtScr Insert Dele 2. LL
Cindy decomposed a metal hydroxide via the reation: Mt(OH) 3 → MtO + H20, and then collected concentration and time data. After analyzing on her TI84 the following data were obtained. [Mt(OH)3] vs. time a = 2.10 x 104 In[Mt(OH)3] vs. time a = -5.80 x 10-5 b = -0.770 r = 0.999 [Mt(OH)3] vs. time a = -1.72 x 10-5 b = 0.450 r = 0.917 2.00 %3D r² 0.981 What is the order with respect to Mt(OH)3? What is the value of the rate constant for this reaction?
Determine the Reaction Order for HCI using calculations described in the background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples, so round to the nearest whole number
Q 18 please
Q 25 please