A laboratory manager performed an experiment to investigate the hydrolysis of 2-chlorooctane at different temperatures. The following results were obtained: Temperature (°C) Rate constant, k, (s-1) | 25 35 45 1.06 x 10-5 | 3.19 x 104 | 9.86 x 104 | 2.92 x 10-3 Using a graphical method, calculate (ii) (iii) pre-exponential factor k value at 50 °C

A laboratory manager performed an experiment to investigate the hydrolysis of 2-chlorooctane at different temperatures. The following results were obtained: Temperature (°C) Rate constant, k, (s-1) | 25 35 45 1.06 x 10-5 | 3.19 x 104 | 9.86 x 104 | 2.92 x 10-3 Using a graphical method, calculate (ii) (iii) pre-exponential factor k value at 50 °C

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

The rate law for the reaction of phenolphthalein with NaOH was determined to be Rate = k[P2−][OH−]. What are the units on the value of the rate constant, k?
Give the reaction mechanism for the following subparts in clear handwritten!
What process of catalysis is 2SO2(g) + O2(g) → 2SO3(g) with V2O5 called?
A solution of 100 g / L of acrylamide in methanol is polymerized at 25 ° C with 0.1 mol / Lof isobutyryl peroxide whose half-life is 9.0 h at this temperature and the efficiency inmethanol is 0.3. For acrylamide, kp2 / kt = 22 L / mol * s at 25 ° C and the termination is onlyby coupling. (a) What is the rate of polymerization, Rp? (b) How much polymer ishave you prepared in the first 10 minutes of reaction in 1 L of solution?
For a certain alkane the activation energies for the rate determining step of fluorination and chlorination are 8.0 kJ/mole and 20 kJ/mole, respectively. Calculate the ratio of the rate of fluorination to that of chlorination at 27oC assuming that the values of A (Arrhenius constant) are the same. (R=8.314 J/mol-K)
When cyclopropane (C3H6) is heated to 500 °C, it turns into propene. The data below were obtained experimentally: a) Indicate the values on the appropriate graph and check the order of reaction in terms of the reagent; b) Confirm that the reaction is 1st order in C3H6 and calculate the rate constant k. Ciclopropano=cyclopropane
The second-order rate constants for the reaction of oxygen atoms ·with aromatic hydrocarbons have been measured (R. Atkinson and J.N . Pitts, J. Phys. Chem. 79, 295 (1975)). In the reaction with benzene the rate constants are 1.44x 107dm' mor ' s ' at 300.3 K, 3.03 x 107 dm' mol"'s"' at 34 1.2K, and 6.9 x 107 dm' mor's ' at 392.2K. Find the frequency factor and activation energy of the reaction.
The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.
if the rate of disapearance of h2o2 is 0.033ms ^-1 what is the rate of appearance of o2? 2h2O2 = 2h2o + o2
The conversion of dissolved carbon dioxide in blood to HCO3- and H3O+ is catalyzed by the enzyme carbonic anhydrase. The Michaelis–Menten constants for this enzyme and substrate are Km = 8 × 10-5 mol L-1 andk2=6 × 105 s-1. (a) What is the maximum rate of reaction of carbon dioxide if the enzyme concentration is 5 × 10-6 M?(b) At what CO2 concentration will the rate of decomposition be 30% of that calculated in part (a)?
Given the 1st order rxn A(g) --- > B(g) + C(g) + 3D(g) with a rate constant of 6.0x10-4 s-1 at 298 K. With a starting mol of 1.00 mol of A(g), how long in seconds does it decrease to 0.500 mol?
An irreversible unimolecular reaction (A -> B) has a rate constant (k) equal to 0.46 s-1. What is the half-time (t1/2)? If at time “zero” the concentration of A is 28 mM, what is the concentration at 1.5 seconds? At 2.17 seconds? Specify your units. t1/2 = [A] at t1/2 = [A] = at t = 2.17 s