Mechanisms and Molecularity7 of 18<>I Review | Constants | Periodic TableOrder and rate law of a reactionLearning Goal:To understand how elementary steps make up amechanism and how the rate law for an elementarystep can be determined.The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because theyare each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementarystep. For example, the rate law for step 1 isVery often, a reaction does not tell us the whole story.For instance, the reactionrate = k[NO2]²The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 isNO2(9) + CO(9)→NO(g)+ CO2(g)rate = k[NO3]"[coj = k[NO3][C0]does not involve a collision between an NO2molecule and a CO molecule. Based on experimentaldata at moderate temperatures, this reaction isthought to occur in the following two steps:because the reaction involves only one molecule of each reactant the exponents are omitted.1. NO2(9) + NO2(g)→NO3(g) + NO(g)2. NO3(9) + C0(g)→CO2(g) + NO2(9)Analyzing a new reactionConsider the following elementary steps that make up the mechanism of a certain reaction:Each individual step is called an elementary step.Together, these elementary steps are called thereaction mechanism.1. 3X-E +F2. E + M F+ NOverall, the resulting reaction isPart ANO2(g) + CO(9)→NO(g)+CO2(9)Notice that in the elementary steps NO3 appears

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Answered: Analyzing a new reaction Consider the…

Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 3X->E +F 2. E + MF+N Bart 0

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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A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H, initial rate of reaction х10 1.26 M 0.560 M 76.0 M/s | M/s 1.26 M 0.272 M | M/s 5.70 M 0.124 M
Consider the following reaction: CaO(s) + CO₂(g) → CaCO3(s) The data found below are the results obtained from using different concentrations of each reactant to measure the initial rate of the reaction: Trial 1 2 3 4 [CaO] (mol L-¹) [CO₂] (mol L-¹) 0.0050 0.0150 0.0200 0.0150 0.0020 O 0.0021 mol L-1 O 0.0042 x 10-² mol L-¹ O 0.4167 mol L-1 O 0.0083 mol L-1 O 0.004 mol L-1 0.0020 0.0040 Determine the concentration of CO₂ during trial 3. Initial Rate (mol L-¹ s-¹) 1.50 × 10-3 0.0135 0.025 0.027
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The following reaction was studied at a given temperature: CH3CI(g) + H20(g) → CH3OH(g) + HCI(g) From the rate data below, determine the reaction orders. Exp [CH3CI]o [H2O]o Initial Rate (M s1) 1 0.100 0.100 0.182 2 0.200 0.200 1.45 3 0.200 0.400 5.81 CH3CI: first order H2O: first order CH3CI: second order H,O: second order CH3CI: second order H,O: first order O CH3CI: first order H2O: second order
Consider this overall reaction, which is experimentally observed to be second order in X and first order in Y: X + Y -----> XY Does the reaction occur in a single step in which X and Y collide and is the two-step mechanism (below) valid?
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Using the data in the table, calculate the rate constant of this reaction. k= = A + B → C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.340 0.400 0.340 0.920 0.408 0.400 Rate (M/s) 0.0114 0.0603 0.0137
Consider the reaction and the information in the table provided. Calculate the average rate of formation of P2O5 between 20.0s and 40.0s. 2H3PO4 → P2O5 + 3H2O Time (s) 0.0 10.0 20.0 30.0 40.0 50.0 Conc P2O5 (M) 0 0.00120 0.00420 0.00600 0.00720 0.00780
3 Use the following kinetic data to determine the order of the reaction and the value of the rate constant. 2NOBr (g) 2 NO (g) + Br2 (g) (8 Time(s) [NOBr] 0 10 20 30 40 0.040 0.030 0.024 0.021 0.018 [18
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[References] This question has multiple parts. Work all the parts to get the most points. a The reaction of NO2 (g) and CO(g) is thought to occur in two steps: Step 1 Slow NO2 (g) + NO2 (9) → NO(g) + N03 (g) Step 2 Fast NO3 (9) + CO(g) → NO2(g) + CO2(g) Add the elementary steps to give the overall, stoichiometric reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
Identify the molecularity of each elementary reaction in the table below. elementary reaction 2NO(g) + Br₂(g) 2NOBr(g) N₂O(g) → N₂(g) + 0(g) CH₂ CH₂ Br(aq) + OH(aq) CH₂CH₂OH(aq) + Br (aq) molecularity Ounimolecular Obimolecular O Cannot be determined. Ounimolecular Obimolecular O termolecular O quadrimolecular O termolecular O quadrimolecular Cannot be determined. unimolecular Obimolecular O Cannot be determined. O termolecular O quadrimolecular X G