Rate of formation of oxygen can be written as A[02]/At for the following reaction. Use this as anexample and write the rate of consumption of N2O5.2 N₂Os (g)->4 NO2 (g) + O2(g)If the rate of formation of oxygen in 0.2 M/s, what is the rate of consumption of N2Os in thisreaction.

Answered: Rate of formation of oxygen can be…

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 11.12PAE: Rank the following in order of increasing reaction rate. (a) Dynamite exploding (b) Iron rusting (c)...

See similar textbooks

Similar questions

The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
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?
Iodomethane (CH3I) is a commonly used reagent in organic chemistry. When used properly, this reagent allows chemists to introduce methyl groups in many different useful applications. The chemical does pose a risk as a carcinogen, possibly owing to iodomethanes ability to react with portions of the DNA strand (if they were to come in contact). Consider the following hypothetical initial rates data: [DNA]0 ( mol/L) [CH3I]0 ( mol/L) Initial Rate (mol/Ls) 0.100 0.100 3.20 104 0.100 0.200 6.40 104 0.200 0.200 1.28 103 Which of the following could be a possible mechanism to explain the initial rate data? MechanismIDNA+CH3IDNACH3++IMechanismIICH3ICH3++ISlowDNA+CH3+DNACH3+Fast
When boron trifluoride reacts with ammonia, the following reaction occurs: BF3(g)+NH3(g)BF3NH3(g)The following data are obtained at a particular temperature: (a) What is the order of the reaction with respect to BF3, NH3, and overall? (b) Write the rate expression for the reaction. (c) Calculate k for the reaction. (d) When [ BF3 ]=0.533M and NH3=0.300M, what is the rate of the reaction at the temperature of the experiment?
Diethylhydrazine reacts with iodine according to the following equation: Â (C2H5)2(NH)2(l)+I2(aq)(C2H5)2N2+2HI(aq)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) What is the order of the reaction with respect to diethylhydrazine, iodine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) What must [(C2H5)2] be so that the rate of the reaction is 5.00104mol/Lh when [ I2 ]=0.500M?
When nitrogen dioxide reacts with carbon monoxide, the following reaction occurs. Â NO2(g)+CO(g)NO(g)+CO2(g)The following data are obtained at a certain temperature: (a) What is the order of the reaction with respect to NO2, CO, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) When [ NO2 ]=0.421Mand [ CO ]=0.816M, what is the rate of the reaction at the temperature of the experiments?
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?
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the 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: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

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: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

Rate of formation of oxygen can be written as A[02]/At for the following reaction. Use this as an example and write the rate of consumption of N2O5. 2 N₂Os (g) -> 4 NO2 (g) + O2(g) If the rate of formation of oxygen in 0.2 M/s, what is the rate of consumption of N2Os in this reaction.