• Part BWhich species is a reaction intermediate?• View Available Hint(s)O EO FO MONSubmitPart CWhat is the rate law for step 1 of this reaction?Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C type k*[A]*[C]*3.> View Available Hint(s)Rate =SubmitPart DWhat is the rate law for step 2 of this reaction?Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][c]* type k*[A]*[C]*3.• View Available Hint(s)Rate =Submit Leaming Goal:To understand how elementary steps make up a mechanism and how the rate law for an elementary step canbe determined.Order and rate law of a reactionVery often, a reaction does not tell us the whole story. For instance, the reactionThe overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in anelementary step. For example, the rate law for step 1 isNO2(9) + CO(g)–→NO(g) + CO2 (9)rate = k[NO2]*does not involve a collision between an NO, molecule and a CO molecule. Based on experimental data atmoderate temperatures, this reaction is thought to occur in the following two steps:The exponent "2" is used because the reaction involves two NOz molecules. The rate law for step 2 is1. NO2(9) + NO2(g)→NO3 (9) + NO(g)2. NO:(g) + CO(g)→CO2(g) + NO2(g)rate = k[NO3]"(COj' = k[NO:]|CO]because the reaction involves only one molecule of each reactant the exponents are omitted.Each individual step is called an elementary step. Together, these elementary steps are called the reactionmechanism.Overall, the resulting reaction isAnalyzing a new reactionNO,(9) + CO(g)-+NO(9) + CO, (9)Consider the following elementary steps that make up the mechanism of a certain reaction:1. 3XE + F2. E+ M→F + NNotice that in the elementary steps NO, appears both as a product and then as a reactant; therefore it cancelsout of the final chemical equation. NO; is called a reaction intermediate. Also notice that 2 molecules of NO2appear in the reactants of the first step and 1 molecule of NOz appears as product of the second step, the neteffect leaves only 1 molecule of NO, as a reactant in the net equation.Molecularity is the proper tem for "how the molecules collide" in a reaction. For example, step 1 is bimolecularbecause it involves the collision of two molecules. Step 2 is also bimolecular for the same reason. Unimolecularreactions involve only one molecule in the reactants. Though rare, collisions among three molecules can occur.Such a reaction would be called femolecular.Part AWhat is the overall reaction?Express your answer as a chemical equation.• View Available Hint(s)Template Symbols undo redo Teset keyboard shortcuts help2x+ 21=m+2zDA chemical reaction does not occur for this question.SubmitPrevlous AnawerePart BWhich species is a reaction intermediate?• View Available Hint(s)O XO EO FO MONSubmit

Answered: Image /qna-images/answer/70b76460-4e98-4567-a3dd-4a5c80aa273b.jpgPlz rate student!!

Part B Which species is a reaction intermediate? > View Available Hint(s) O X O E O F O M ON Submit • Part C What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][c}* type k*[A]*[C]*3. • View Available Hint(s) Rate = Submit • Part D What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A]|c* type k*[A]*[CJ*3. • View Available Hint(s) Rate = Submit

Part B Which species is a reaction intermediate? > View Available Hint(s) O X O E O F O M ON Submit • Part C What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][c}* type k[A][C]3. • View Available Hint(s) Rate = Submit • Part D What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A]|c type k[A][CJ*3. • View Available Hint(s) Rate = 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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For elementary reactions, rate equations can be written directly from the stoichiometry True O False
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The rate constant (k) for a reaction was measured as a function of temperature. A plot of In k versus 1/T (in K) is linear and has a slope of - 6704 K. Calculate the activation energy for the reaction. Express your answer to four significant figures and include the appropriate units. ? J E, 5.570 10 mol Submit Previous Answers Bequest Answer X Incorrect; Try Again; 3 attempts remaining
For the reaction mechanism below answer the questions. Fast equilibrium OH- + O2NNH2 --> O2NNH- + H2O Slow O2NNH- --> N2O + OH- c. What is the predicted rate law?
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Can someone please help with question 11 a and b
O KINETICS AND EQUILIBRIUM Using a second-order integrated rate law to find concentration... -1-1 At a certain temperature the rate of this reaction is second order in Cl,0, with a rate constant of 103.Ms: 2Cl,0; (g) 2Cl, (g) +50, (g) → Suppose a vessel contains Cl,0, at a concentration of 0.130M. Calculate the concentration of Cl,0, in the vessel 0.550 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10 Check Explanation Terms of Use | Privacy Center Accessibility 2021 McGraw Hill LLC. All Rights Reserved. II
Hi i am having trouble with this portion of the question. Please provide handwritten solution for better understanding CO(g) + Cl2(g) COCl2(g) The above reaction obeys the mechanism: Cl2 --> 2Cl Fast equilibrium Cl + CO--> COCl Fast equilibrium COCl + Cl2 --> COCl2 + Cl Slow 2Cl--> Cl2 Fast 1b) Suppose that: k1/k-1 = 1×10-2 mol L-1, k2/k-2 = 1×106 L mol-1, k3 = 1×10-4 L mol-1 s-1, and k4 = 1×103 L mol-1 s-1. What would be the value of the overall rate constant, k, including the correct units?
Captain Marvelibrium discovered a figure with data frorh an experiment left by Le Châtelier Flipdime. Consider the following data where A andB are mixed at initial concentrations indicated. Upon reacting the concentrations change a can be read from the plot. The reaction is A(g) + B(g) = C(g). C Time (s) Based on figure, calculate the value for Ke for the reaction. Submit Answer Tries 0/99 This discussion is closed. Send Feedback MAR 10 étv МacВос Air 000 esc F1 F2 F3 F4 F5 F6 #3 $4 3. 4 CO AB 3. Concentration (mol.dm-3)
t- Assignme... Connect P Course Home E Login | Student Veri... Bb Logout MyProgrammingLab Im O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [-] [H.] , initial rate of reaction 1.75 M 0.767 M 16.0 M/s 7.77 M 0.767 M 71.0 M/ s 1.75 M 0.136 M 2.84 M/ s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k D k = ]
Show all working explaining detailly each step. Answer should be type written using a comuter Keyboard!