Experiment shows that the rate formation of carbon tetrachloride from chloroform,CH3 +Cl2 → CCl4 + HCIis the first order in CHCl3, ½ order in Cl2 and 3/2 order overall. Is the followingmechanism consistent with the overall rate low?Cl2 2 Cl(K1, K-1)fastCl + CHCl 3 → HCI + CC13⚫(k2)slowCCl3 + Cl⚫CCl4(K3)fast(Use the steady state principle for the radicals Cl• and CC13. to determine thedifferential rate equation of carbon tetrachloride formation d [CCl4] / dt).

Step 1:To determine if the proposed mechanism is consistent with the observed rate law, let's…

Answered: Experiment shows that the rate…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 12Q: The plot below shows the number of collisions with a particular energy for two different...

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Which of the following will confirm that the decomposition of SO2Cl2 (to form SO2 and Cl2) is a first-order process? (a) A graph of [SO2Cl2] vs. time gives a curved line. (b) A graph of ln[SO2Cl2] vs. time gives a curved line. (c) A graph of 1/[SO2Cl2] vs. time gives a straight line. (d) A graph of ln[SO2Cl2] vs. time gives a straight line.
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
There are two molecules with the formula C3H6 Propane, CH3CH = CH2, is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anesthetic: When heated to 499 C, cyclopropane rearranges (isomerizes) and forms propane with a rate constant of 5.95104s1. What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499 C?
The rate constant for the ?rst-order decomposition at 45 C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCI3, is 6.2104 min-1. 2N2O54NO2+O2 What is the rate of the reaction when [N2O5] = 0.40 M?
The rate constants for the ﬁrst order reaction were found at different temperatures (below). What is theactivation energy for this reaction in kJ/mol? T1 = 11.6 oC k1 = 0.35 T2 = 48.6 oC k2 = 7.1Report your answer to the nearest whole number.
Rate law = k [HgCl2] [C2O4 -2]^2 I believe k = 0.022584815 s^-1 d. What is the rate of disappearance of oxalate ion when [C2O2−4]= 0.10 M[C2O42−]= 0.10 M and [HgCl2] = 0.20 M[HgCl2] = 0.20 M? e. Is the overall reaction likely to be an elementary step? Explain. f. Which species is oxidized in the reaction? Which is reduced?
Part A: Based on the energy diagram, determine which step is rate limiting. Answer: The first step Part B: What is the rate law of the reaction in part A? Part C: What is the order of the reaction based on the answer to part B?
What is the rate law for the proposed mechanism? A) rate = k[H2][NO] H2(g) + 2NO(g) → N2O(g) + H2O(g) k[H•J°[NO] Step 1 (slow) B) rate = rate = k[H:][NO]? %3D N20(g) + H2(g) –→ N2(g) + H2O(g) Step 2 (fast) D) rate = k[H:]°[NO]? E) rate = k[H:][N:O]
Options for part a: Unimolecular, bimolecular, termolecular
The reaction H2S (g) + Br2 (g) → S (s) + 2 HBr (g) is second order for Br2. Which of the following "Trial 2" data will support this reaction order for bromine? Trial [H2S] (M) [Br2] (M) rate (MS-1) 1 0.02 0.04 1.12 x 10-3 2 ??? ??? ??? [H2S] = 0.02 M; [Br2] = 0.08 M; rate = 2.24 x 10-3 M s-1 [H2S] = 0.04 M; [Br2] = 0.04 M; rate = 1.12 x 10-3 M s-1 [H2S] = 0.02 M; [Br2] = 0.08 M; rate = 4.48 x 10-3 M s-1 [H2S] = 0.02 M; [Br2] = 0.04 M; rate 1.12 x 10-3 M s 1 =
CHAP 14 EXERCISES 1- 2 A few drops of blue food dye were added to water followed by a solution of bleach. (Initially, the concentration of dye was about 3.4 x 10-5 M and the bleach (NaOCI) concentration was about 0.034 M.) The dye 3.50 3.00 2.50 2.00 1.50 1.00 faded as it reacted with the bleach. The color 0.50 change was followed by a spectrophotometer, and the data values are plotted below. With time, does the rate of reaction decrease, stay the same, or 0.00 3 5 Time (min) increases? The reaction of CH;COOH(aq) with NaHCO3(s) generates CO,(g). The reactants are mixed in a sealed 500.0-mL vessel. After 30.0 minutes, 2.55 x 10-3 mol CO, has been generated. Calculate the average rate of the reaction.
A+B⟶C+Drate=?[A][B]2A+B⟶C+Drate=k⁡[A]⁢[B]2 has an initial rate of 0.0790 M/s.0.0790 M/s. What will the initial rate be if [A][A] is halved and [B][B] is tripled?

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