Given the following mechanism: NO(9) • Fag) <> NO,F:(g) NO Fg) NO,F(g) + F(g) Fig) NO,(g) → NO F(9) (fast) (slow) tast) (a) Write the overall reaction, Show your answer (b) Mentions the intermediaries: (c) Show whether the proposed mechanism is consistent with the overal reaction whose rate of reaction is kNO J[F].

Given the following mechanism: NO(9) • Fag) <> NO,F:(g) NO Fg) NO,F(g) + F(g) Fig) NO,(g) → NO F(9) (fast) (slow) tast) (a) Write the overall reaction, Show your answer (b) Mentions the intermediaries: (c) Show whether the proposed mechanism is consistent with the overal reaction whose rate of reaction is kNO J[F].

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter13: Kinetic Methods

Section: Chapter Questions

Problem 4P

See similar textbooks

Similar questions

For the simplest serial first order reactions A→ R→S; the concentration of componentA -increases continuously with timeB-Rincreases continuously with timeC-Sincreases continuously with timeD-R decreases to a minimum and then increases continuously with time
Give the reaction mechanism for the following subparts in clear handwritten!
1. The following initial rate data are for the ozonization of pentene in carbon tetrachloride solution at 25 oC:C5H10 + O3 C5H10O3 Experiment [C5H10]o, M [O3]o, M Initial Rate, Ms-1 1 6.32×10-2 1.34×10-2 76.0 2 6.32×10-2 2.68×10-2 152 3 0.126 1.34×10-2 151 4 0.126 2.68×10-2 303 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is ________ M-1s-1.
please include explanations and mechanisms
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.
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 the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NHẠNCO__(NH2)2CO the following data have been obtained: [NHANCO], M 0.375 time, min 0 0.153 5.88 9.59×10-2 11.8 6.98×10 2 17.6 The average rate of disappearance of NH4NCO over the time period from t = 5.88 min to t = 11.8 min is
Explain the Mechanism of reaction. ASAP
Complete the mechanism for the reaction of 2‑butanol in sulfuric acid at 140 °C. Sulfuric acid is abbreviated as H+H+ in the drawing module. In Step 3, the generic alcohol ROHROH represents another 2‑butanol molecule?
Give the organic chemical reaction mechanism of the synthesis of 1-bromobutane. link of the video in making 1-bromobutane: https://www.youtube.com/watch?v=bgTu3_05HsI
The degradation of the antibiotic clindamycin stored at 343 K in aqueous solution at pH 4 is found to be first order with a rate constant of 2.49 x 10−7 s −1. Over the temperature range 320 K to 360 K theactivation energy was found to be 123.3 kJ mol−1. (a) Calculate the rate constant at 325 K.(b) The threshold for product safety is 1% degradation. At 295 K the time taken for 1% of the antibiotic to degrade is found to be close to 0.01/ k. Comment on the shelf-life of the drug.
The ha lf-l ife of pyruvic acid in the presence of an aminotransferaseenzyme (which converts it to alanine) was found to be 221 s. How long will it take for the concentration of pyruvic acid to fal l to 1/ 64 of its in it ial va lue in th is first-order reaction?