Consider the following multistep reaction:А +В АВ (slow)A + AB→A,B (fast)2A + B А2в (overall)Based on this mechanism, determine the rate law for the overall reaction.Express your answer in standard MasteringChemistry format. For example, if the rate law isk[A]°[B]? type k* [A]^3* [B]^2.• View Available Hint(s)Submit Part BConsider the following multistep reaction:C+D = CD (fast)CD + D →CD2 (slow)CD2 + D→CD3 (fast)C+ 3D →CD3 (overall)Based on this mechanism, determine the rate law for the overall reaction.Express your answer in standard MasteringChemistry format. For example, if the rate law isk[C]³ [D]? type k* [C]^3* [D]^2.· View Available Hint(s)Submit

Rate law is always written by the slowest step. In first reaction slowest step is :- A + B…

Consider the following multistep reaction: C+D = CD (fast) CD + D →CD2 (slow) CD2 +D→CD3 (fast) C+ 3D →CD3 (overall) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C]³ [D]² type k*[C]^3*[D]^2. • View Available Hint(s) Submit

Consider the following multistep reaction: C+D = CD (fast) CD + D →CD2 (slow) CD2 +D→CD3 (fast) C+ 3D →CD3 (overall) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C]³ [D]² type k[C]^3[D]^2. • View Available Hint(s) Submit

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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= ○ KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi... Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H₂ (g) + 2NO(g) → N₂O(g) + H₂O(g) k₁ 2 H₂(g) + N₂O(g) → N₂ (g) + H₂O(g) K₂ Suppose also k₁ <
Let’s consider the following reaction, X+2Y - Z After performing some experiments, let’s assume a researcher has determined the rate law for this reaction to be, Rate = k [X][Y]2 But later, a second researcher reports that the mechanism for this reaction is actually, 2Y- 1 (slow) X+1- Z (fast) In the previously determined rate law consistent with this mechanism? If not, why? What should be rate law predicted by this mechanism?
1) NO(g) + O2 (g) >< NO3 (g) 2) NO3(g) + NO(g) > < 2NO2(g0 for the reaction mechanism given, what is the rate law for each elementary equation? What is the rate law for the overall reaction if the mechanism is correct?
The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)
Click in the answer box to activate the palette. Enter the general form of the rate law for the following process. Represent the order as n, n', and so forth. Complete the equation using brackets, [], to represent concentration. 2Cu(g) + O2(g) → 2CuO(g)
Suggest a mechanism behind the reaction NO(g) + Cl2(g) à NOCl(g) + Cl(g) with the rate law rate = k [NO]2 [Cl2] This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2 (slow) 2NO + Cl2 à ………. (fast). à ………… NO + Cl2. à NOCl + Cl
Reaction of nitric oxide gas (NO) and chlorine gas (Cl2) produces a very poisonous gas called nitrosyl chloride (NOCl). The experimental data of the reaction is given below. Use the data to calculate the specific rate constant K and overall order of the reaction. Please show full work!
Q2) Consider the following third order reaction: A➜ product The following is the integrated rate law for the third order reaction: 2[A];² 11/2 = kt + 1.5 K[A]0² 2[A]o² If the concentration of the reactant after 26.5 second of the experiment was found to 0.348 M and the rate constant for this reaction was found to be 1.5x10¹² M².S¹. a) Determine the initial concentration of the reactant. b) What is the half-life of this reaction? c) What is the concentration of the reactants after 1.00 min of the experiment?
The half-life of a reaction, t/2. is the time it takes for the reactant concentration A| to decrease by half. For example, after one half-life the concentration falls from the initial concentration [Alo to [Alo/2, after a second half-life to [A]o/4, after a third half-life to [Alo/8. and so on. on.
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