Identify the molecularity of each elementary reaction in the table below.elementary reaction2NO(g) + Br₂(g) 2NOBr(g)N₂O(g) → N₂(g) + 0(g)CH₂ CH₂ Br(aq) + OH(aq) CH₂CH₂OH(aq) + Br (aq)molecularityOunimolecularObimolecularO Cannot be determined.OunimolecularObimolecularO termolecularO quadrimolecularO termolecularO quadrimolecularCannot be determined.unimolecularObimolecularO Cannot be determined.O termolecularO quadrimolecularXG

Identify the molecularity of the given reactions.

Identify the molecularity of each elementary reaction in the table below. elementary reaction 2NO(g) + Br₂(g) 2NOBr(g) N₂O(g) CH₂CH₂ Br(aq) + OH (aq) N₂(g) + O(g) CH₂CH₂OH(aq) + Br (aq) molecularity Ounimolecular Obimolecular O termolecular O quadrimolecular Cannot be determined. Ounimolecular Obimolecular O termolecular O quadrimolecular Cannot be determined. O termolecular O quadrimolecular Ounimolecular Obimolecular O Cannot be determined. X

Identify the molecularity of each elementary reaction in the table below. elementary reaction 2NO(g) + Br₂(g) 2NOBr(g) N₂O(g) CH₂CH₂ Br(aq) + OH (aq) N₂(g) + O(g) CH₂CH₂OH(aq) + Br (aq) molecularity Ounimolecular Obimolecular O termolecular O quadrimolecular Cannot be determined. Ounimolecular Obimolecular O termolecular O quadrimolecular Cannot be determined. O termolecular O quadrimolecular Ounimolecular Obimolecular O Cannot be determined. X

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.82PAE

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Similar questions

Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
. explain the difference between elementary reactions and multistep reactions.
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.