N-nitrosodimethylamine (NDMA) is a suspected carcinogen that can form via reactionsbetween dimethylamine (DMA) and monochloramine (NH2Cl). The relevant elementaryreactions and the corresponding rate constants are as shown below.ReactionRate constant (M¹s¹)DMA + NH2Cl = DMCA + NH3k =1.4×10-1, kr = 5.83×10-31.28×10-3DMA + NH2Cl → UDMHUDMH + NH2Cl → NDMA->1.11×10-1If the initial concentrations of DMA and NH2Cl are given, you should be able to predict theconcentrations of all species at any given reaction time. Please write down the rate equationsfor DMA, NH2C1, DMCA, UDMH and NDMA.

Answered: Image /qna-images/answer/30a9479e-9204-4948-ad98-b75461679581.jpg

Answered: N-nitrosodimethylamine (NDMA) is a…

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

Calculate the rate of the reaction (k) of ∙OH (105 molecules cm-3) with atmospheric CO (150 ppb) at 28°C, given that the rate constant for the process is 5 × 10-13 exp (-300 / temp) molecule-1 cm3 s-1.
Given the transition state diagram(s) below, identify the mechanism(s) of catalysis. Mg2+ Mg2+ H OH H-C-H HOH H H - (M₂C)N= H H-C-H HO -H H- HO -H OH-O -O-H- H-N(CH₂) CH₂OH H H₂C H H LN (CH2) H OH HOH:N (0³H)² CH₂OH H₂C t
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.
Suggest a reaction mechanism
An excited ozone molecule, 03*, in the atmosphere can undergo one of the following reactions, Оз (1) fluorescence 03 O + 02 (2) decomposition 03" + M - 03 + M (3) deactivation, where M is an inert molecule, the rate constant for the fluorescence reaction is k1, the rate constant for the decomposition reaction is k2, and the rate constant for the deactivation reaction is k3. Write a simplified expression for the fraction, X, of ozone molecules undergoing decomposition in terms of the rate constants. (Use the following as necessary: k1, k2, k3, co for [03*], and CM for [M].) X =
ΚΗ Consider the following reaction which has the observed kinetic isotope effect = 1.5. kD Cy2 "PH Δ Cy2 -PI...pt + -P Cy2 Cy2 A) Draw a mechanism for this reaction and identify the type of reaction which is occurring.
I'm not really sure how to approach this problem. I thought you could substitute the half life equation into the integrated equation for first order reactions, but that didn't work.
For the gas phase decomposition of acetic anhydride, (CH3CO) 20→ CH₂=C=O + CH3COOH the rate constant at 502 K is 1.02 x 10³ s1 and the rate constant at 551 K is 0.0219 s¹. The activation energy for the gas phase decomposition of acetic anhydride is kj.
Payalben
k1 The mechanism A + A A2* A2* + M k2 K2 A2+ M k.1 is common in reactions of the type A + A + M → A2 + M. Is it correct? Explain it.
In a research paper, (Orkin et al., J. Phys. Chem., 1997, 101: 174) rate constants were determined for the reaction between the hydroxyl radical and chlorobromomethane: OH• + CH2BrCI → products Data that were obtained included the following values of the rate constant k for the following temperatures: Т, К k, cm³/molecule•sec 298 1.11 x 10 13 313 1.34 x 10 13 330 1.58 x 10 13 Determine the E, and the pre-exponential factor. E = J/mol A = cm3/molecule•sec
Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 CH33CBr (aq) → CH33C+ (aq) + Br− (aq) k1 2 CH33C+ (aq) + OH− (aq) → CH33COH (aq) k2 Suppose also k1 ≫ k2 . That is, the first step is much faster than the second.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS