Find the rate law for the reaction 2 N205(g) → 4 NO2(g) + O2(g) based on the proposed mechanism:N205NO2 + NO3fastNO2 + NO3NO + N205NO2 + 02 + NOslow3 NO2fastrate = k[ N205]°rate = k[ N205)?rate = k[ NO2][ NO3]O rate = k[ N205]

The rate of the overall reaction depends on the rate of the slow step only. Therefore, the rate law…

Find the rate law for the reaction 2 N205(g) – 4 NO2(g) + O2(g) based on the proposed mechanism: NO2 + NO3 NO2 + O2 + NO - 3 NO2 N205 fast NO2 + NO3 NO + N205 slow fast O rate = k[ N205)° rate = k[ N2O5)? O rate = k[ NO2][ NO3] O rate = k[ N205) %3D

Find the rate law for the reaction 2 N205(g) – 4 NO2(g) + O2(g) based on the proposed mechanism: NO2 + NO3 NO2 + O2 + NO - 3 NO2 N205 fast NO2 + NO3 NO + N205 slow fast O rate = k[ N205)° rate = k[ N2O5)? O rate = k[ NO2][ NO3] O rate = k[ N205) %3D

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 31QRT

See similar textbooks

Related questions

Q: 3. What is the total reaction order of the following rate law equation: = k[A]*[B]°[C]? a) 0 b) 1 c)…

A: To find: The order of the reaction, rate = k[A]1[B]0[C]2

Q: A first-order reaction has a rate constant of 0.33 min−1. It takes ________ min for the reactant…

Q: The reaction, 2 A2X4(g) → 2 A2X3(g) + X2(g), was found to be first order. The rate law,…

A: In this question, we will see the rate law equation for the given first order reaction. You can see…

Q: n the chemistry lab, you’re asked to determine the mechanism for the following reaction: CH3CHBrCH3…

Q: What rate law corresponds to the mechanism? 2NO(g) 2 N202(g) k; k.1 fast H2(8) + N2O2(g) H2O(g)…

Q: A reaction is determined to have the rate law rate = k[NO]°[H,]. What is the rate- determining step…

A: We have to determine the slowest step of the reactions.

Q: What is the absolute magnitude of the rate of change for [NH₃] if the rate of change for [H₂] is…

Q: Consider the following chemical equation: Overall Reaction: 2AB +2C2 - A2 + 2C,B The proposed…

A: Rate law : Rate law is the expression which gives rate of reaction interms of molar concentration…

Q: What is the absolute magnitude of the rate of change for [NH₃] if the rate of change for [H₂] is…

A: For the reaction: 2 NH₃(g) → N₂(g) + 3 H₂(g) The differential rate can be written as follows:…

Q: What would be the rate law for the mechanism below? Step 1 NO(g) + Cl2(g) ↔ NOCl2(g) slow Step 2…

A: The given equations are : Step 1 NO(g) + Cl2(g) ↔ NOCl2 (g) slow Step 2…

Q: Consider the proposed mechanism for the reaction, CHCl3(g) + Cl2(g) --> HCl(g) + CCl4(g)…

A: Consider the proposed mechanism for the reaction, A student proposes that the reaction rate law…

Q: 1. Nitric oxide, NO, and hydrogen gas react though the following reaction: 2NO(g) + 2H2(8) → N2(®) +…

Q: Consider the overall reaction: АВ + С А+ Bс And its proposed mechanism: AB + AB → AB2 + A slow АВz +…

A: Rate law of a reaction is determined by RDS i.e rate determining step and slowest step is rate…

Q: Nitryl bromide, NO2Br, decomposes into nitrogen dioxide and bromine. 2NO2Br(g) → 2NO2(g) + Br2(g)…

Q: Consider the following chemical equation: Overall Reaction: A3B + AC - A2B + C+ A2 The proposed…

A: Rate equation for the general reaction A+B--->Product is, The rate of the reaction is…

Q: Consider the following three-step mechanism for a reaction: Cl2 (g) = 2 CI (g) Fast CI (g) + CHCI3…

A: The rate law of the reaction is given by,

Q: One proposed mechanism for the decomposition of N205 to NO2 involves three elementary steps: Step 1:…

A: Given R x n is in question If we add all three equation , we get overall r x n = 2N2O5→4NO2+O2…

Q: The reaction of A + B +C = ABC occurs in three elementary steps: Step 1: A + B → AB Step 2: AB + С ~…

A: Slow step is rate determining step

Q: What would be the rate law for the mechanism below? Step 1 I2 → 2 I fast Step 2 2 I + H2 ↔ 2 HI…

A: The rate law of a reaction is determined experimentally. The sum of the exponent term in the rate…

Q: Consider the reaction A + B products with the following rate law: rate = k[A]²[B] Which of the…

Q: Overall Reaction: A2 + B2 → 2 AB The proposed mechanism is as follows: A2 ⇋ 2A (fast) 2A + B2…

Q: Consider this net or overall reaction. KY + Z X + YZ What is the rate law for the reaction based on…

Q: The mechanism for the reaction 2 H2O2(aq) → 2 H2O(1) + O2(g) in the presence of I(aq) is proposed to…

A: Rate laws for reactions are affected by the position of the rate-determining step in the overall…

Q: The mechanism for the reaction 2 H2O2(aq) → 2 H2O(1) + O2(g) in the presence of I (aq) is proposed…

Q: Consider the proposed mechanism. What is the rate-determining step? Step 1: N205 NO2 + NO3 (fast)…

A: Given,

Q: One of the reactions that occurs in polluted air in urban areas is 2NO2(3) + O3lg) → N2O5(3) +…

Q: What is the absolute magnitude of the rate of change for [NH₃] if the rate of change for [H₂] is…

A: The reaction taking place is given as, => 2 NH₃(g) → N₂(g) + 3 H₂(g) Given: Rate of change for…

Q: NH4+(aq) + NO2-(aq) N2(g) + 2H2O(l) EXPT [NH4+] [NO2-] RATE 1 0.010 M…

A: The reaction and the generalized equation for rate law is shown as follows:

Q: Given the following proposed mechanism, predict the rate law for the overall reaction: 2 NO2 + Cl2…

Q: Suppose the reaction 2AB + C2→A 20 +B 20 occurs by the following mechanism. AB Step 1 Step 2 Step 3…

A: In any multi-step reaction, the slowest step is the rate determining step. Rate law of reaction…

Q: Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2…

A: Rate of any reaction depends on the slowest step of the reaction. Hence the rate of slowest step of…

Q: The initial concentration of a reactant A in a second order reaction is 0.8 M. What will be the…

A: Given: Initial concentration of reactant A = 0.80 M Order of the reaction = 2 And the time passed =…

Q: A particular reaction is found to be first order. The reactant has an initial concentration of 2.88…

A: Based on the kinetic facts, the reactions can be classified based on the order. Reactions can be…

Q: The mechanism for NO2 (g) + CÓ (g) → NO (g) + CO2 (g) is thought to be: 2 NO2 NO3+ NO NO3 + CO NO2+…

Q: If the reaction 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) is first order in H2 and first order in…

A: Order of a reaction is the sum of stoichiometric coefficients which are present in the power of the…

Q: Step 1: NO2(g) + F2(g) →NO2F(g) + F(g) slow Step 2: F(g) + NO2(g) → NO2F(g) fast 10. If the…

Q: The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be…

Q: Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO2 + Cl2 →…

A: If the reaction goes via more than one step then the rate depends on the slowest step of the…

Q: Of the three mechanisms listed below, which mechanism agrees with the overall reaction and…

Q: Ellie Mint is trying to determine the reaction mechanism for the following reaction: 2 H2 + 2 NO—>N2…

A: The rate law of a reaction is determined by the slowest step of reaction. The sum of molecularity of…

Q: The reaction of NO gas with H2 gas has the following rate law: Rate = k[H2][NO]2. A proposed…

A: Since we can see that in reaction step 1 we habe 1 H2 and 2 NO molecules reacting And since…

Q: What is the absolute magnitude of the rate of change for [NH₃] if the rate of change for [H₂] is…

Q: Given the following two-step mechanism for a certain reaction: 2 NO(g)→ N2O2(g) (slow) N2O2(g) +…

A: Rate law is a mathematical relationship obtained by comparing the reaction rate with reaction…

Q: The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A…

A: The rate law for the 1st reaction is:Rate = k [NO] [Cl2] The rate law for the 2nd reaction mechanism…

Q: Overall Reaction: A2 + BC4 → AB + AC4 The proposed mechanism is as follows: A2 ⇋ 2A (fast) A +…

A: Given Reaction: A2 + BC4 → AB + AC4 Rate law: The rate of the reaction is expressed as function of…

Q: What is the overall reaction, the rate law and order of reaction? 2N2O5(g) 4NO2(g) + O2(g) N2O5 NO2…

A: Given reaction,

Q: What is the rate law of the reaction NO2(g) + CO(g) ó NO(g) +…

A: Given overall reaction is : NO2 (g) + CO (g) ---------> NO (g) + CO2 (g) Mechanism is : Step.1…

Q: A2 -> 2A (slow) 2A + B2 -> 2AB (fast) What is the rate law for the overall reaction?

A: Given, A2 -> 2A (slow) 2A + B2 -> 2AB (fast)

Q: 9. The reaction of A + B + C = ABC occurs in three elementary steps: Step 1: A + B -> АВ Step 2: AB…

Q: A proposed mechanism for the gas phase reaction of chloroform (CHCl3) and chlorine is as follows: 1.…

A: The relation between the concentration of the reactants and the rate of reaction is expressed by the…

Question

Find the rate law for the reaction 2 N205(g) → 4 NO2(g) + O2(g) based on the proposed mechanism:
N205
NO2 + NO3
fast
NO2 + NO3
NO + N205
NO2 + 02 + NO
slow
3 NO2
fast
rate = k[ N205]°
rate = k[ N205)?
rate = k[ NO2][ NO3]
O rate = k[ N205]

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Hydrogen peroxide, H2O2(aq), decomposes to H2O() and O2(g) in a reaction that is first-order in H2O2 and has a rate constant k = 1.06 103 min1 at a given temperature. (a) How long will it take for 15% of a sample of H2O2 to decompose? (b) How long will it take for 85% of the sample to decompose?
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
The catalyzed decomposition of hydrogen peroxide is first-order in [H2O2]. It was found that the concentration of H2O2 decreased from 0.24 M to 0.060 M over a period of 282 minutes. What is the half-life of H2O2? What is the rate constant for this reaction? What is the initial rate of decomposition at the beginning of this experiment (when [H2O2] = 0.24 M)?
Gaseous azomethane, CH3N=NCH3, decomposes in a first-order reaction when heated: CH3N=NCH3(g) N2(g) + C2H6(g) The rate constant for this reaction at 600 K is 0.0216 min1. If the initial quantity of azomethane in the flask is 2.00 g, how much remains after 0.0500 hour? What mass of N2 is formed in this time?
The decomposition of SO2Cl2 is a first-order reaction: SO2Cl2(g) SO2(g) + Cl2(g) The rate constant for the reaction is 2.8 103 min1 at 600 K. If the initial concentration of SO2Cl2 is 1.24 103 mol/L, how long will it take for the concentration to drop to 0.31 103 mol/L?
In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were obtained: Initial Concentration of Azomethane Initial Rate Exp. 1 1.13 102 M 2.8 106 M/s Exp. 2 2.26 102 M 5.6 106 M/s What is the rate law? What is the value of the rate constant?
The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
Nitryl fluoride is an explosive compound that can be made by oxidizing nitrogen dioxide with fluorine: 2 NO2(g) + F2(g) → 2 NO2F(g) Several kinetics experiments, all done at the same temperature and involving formation of nitryl fluoride, are summarized in this table: Write the rate law for the reaction. Determine what the order of the reaction is with respect to each reactant and each product. Calculate the rate constant k and express it in appropriate units.
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).
Gaseous azomethane (CH3N2CH3) decomposes to ethane and nitrogen when heated: CH3N2CH3(g) CH3CH3(g) + N2(g) The decomposition of azomethane is a first-order reaction with k = 3.6 104 s1 at 600 K. (a) A sample of gaseous CH3N2CH3 is placed in a flask and heated at 600 K for 150 seconds. What fraction of the initial sample remains after this time? (b) How long must a sample be heated so that 99% of the sample has decomposed?
The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2: Step 1: Slow NO2(g) + NO2(g) NO(g) + NO3(g) Step 2: Fast NO3(g) + CO(g) NO2(g) + CO2(g) (a) Show that the elementary steps add up to give the overall, stoichiometric equation. (b) What is the molecularity of each step? (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? (d) Identify any intermediates in tins reaction.
The decomposition of nitrogen dioxide at a high temperature NO2(g) NO(g) + O2(g) is second-order in this reactant. (a) Determine the rate constant for this reaction if it takes 1.76 min for the concentration of NO2 to fall from 0.250 mol/L to 0.100 mol/L (b) If the chemical equation is written as 2 NO2(g) 2 NO(g) + O2(g) what is the value of the rate constant?