Consider the zeroth order decomposition of A with an initial concentration of 5.5 M.If k= 0.0460 s what is the concentration of A after 5 seconds?Your Answer:AnswerunitsQuestion 29 (1 point)ListenWhat is the rate order for a chemical reaction with the rate law: rate = k[B]?a) 3b) 1c) 2d) OQuestion 30 (1 point)ListenConsider a first order decomposition reaction of A witht1/2 = 85 seconds. If theinitial concentration was 2.50 M, what is the final concentration after 110 seconds?(Hint: Calculate k using the half-life equation, then use the correct integrated ratelaw.)Your Answer:Answerunits

Answered: Image /qna-images/answer/a627eb8a-cd09-40dc-9b37-56a2a57336e2.jpg

Answered: Consider the zeroth order decomposition…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.64PAE: 11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed...

See similar textbooks

Similar questions

A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
The decomposition of nitrosyl chloride was studied: 2NOCl(g) 2NO(g) + Cl2(g) The following data were obtained where Rate=[NOCl]t [NOCl]0(molecules/cm3) Initial Rate (molecules/cm3 s) 3.0 1016 5.98 104 2.0 1016 2.66 104 1.0 1016 6.64 103 4.0 1016 1.06 105 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the value of the rate constant when concentrations are given in moles per liter.
3. The equation for the decomposition of NO2(g) at 573 K is 2 NO2(g) → 2 NO(g) + O2(g). Using the concentration-time data below, determine the order of the reaction with respect to [NO2]. [NO2], m Time, min 0.20 0 0.095 5 0.063 10 0.047 15 first-order second-order zero-order
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
The decomposition of sulfuryl chlorideSO2Cl2fur dioxide and chlorine gases is a first-order reaction. It is found that at a certain temperature, it takes 1.43 hours to decompose 0.0714 M to 0.0681 M. (a) What is the rate constant for the decomposition? (b) What is the rate of decompostion [ SO2Cl2 ]=0.0462M? (c) How long will it take to decompose SO2Cl2 so that 45% remains?
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earths ozone layer. The table below lists several (second-order) reactions of Cl atoms with ozone and organic compounds; each is given with its rate constant. For equal concentrations of Cl and the other reactant, which is the slowest reaction? Which is the fastest reaction?
Which of the following statement(s) is( are) true? a. The half-life for a zero-order reaction increases as the reaction proceeds. b. A catalyst does not change the value of the rate constant c. The half-life for a reaction, aAProducts that is first order in A increases with increasing [A]0. d. The half-life for a second-order reaction increases as the reaction proceeds.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
What is the difference between average rate, initial rate, and instantaneous rate?
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry for Engineering Students

Chemistry

ISBN:

9781285199023

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry for Engineering Students

Chemistry

ISBN:

9781285199023

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS