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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The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results: Experiment [HBr(g)] (M) [O2(g)] (M) Rate (M/s) 1 0.00542 0.00542 0.341 2 0.00542 0.0108 0.679 3 0.0108 0.00542 0.679 4 0.0108 0.0108 1.35 (a) What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)] Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2 Rate = k [HBr(g)]2 [O2(g)]2 Rate = k [HBr(g)] [O2(g)]3 Rate = k [HBr(g)]4 [O2(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of HBr(g) is 0.00861 M and that of O2(g) is 0.0123 M if the temperature is the same as that used to obtain the data shown above? _________M/s
Using the following data below for the generic reaction A + B --> 2C + D , which obeys the rate equation d[D]/dt=k[A]α[B]β [A] (M) [B] (M) d[D]/dt (M/s) 0.300 0.300 1.31×10−5 0.600 0.300 3.69×10−5 0.300 0.600 1.85×10−5 a. What are the orders with respect to A and B (α,β)? What is the overall reaction order? b. What is the value of the rate constant k? Be sure to include units. c. Collecting concentration vs. time data would be another possible method to determine k. Describe and sketch the way you would plot these data to obtain a linear relationship, and how you would determine k based on this plot.
A reaction between substances A and B has been found to give the following data: [A] (mol/L) 1.0×10-² 1.0×10-² 2.0×10-² 2.0×10-² 3.0×10-² 3A + 2B > 2C+D [B] (mol/L) 1.0 3.0 3.0 1.0 3.0 Rate of appearance of C (mol/L-hr) 0.300×10-6 8.10×10-6 3.24x10-5 1.20×10-6 7.30×10-5 Using the above data, determine the order of the reaction with respect to A and B, the rate law, and calculate the specific rate constant.
A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? 1 st step: A + B --> 2C + D slow2 nd step: C --> E fast3 rd step: D --> 2F fast rate = k [E] [F]2 rate = k [E] rate = k [C]2 [D] rate = k [C] rate = k [A] [B]
For the following reaction Mechanism write the overall reaction and write the rate law. H3O++ I- → HI + H2O (fast) H2O2 + HI → H2O + HOI (fast) HOI + H3O++ I- →2H2O + I2 (slow) I2 + I- → I3-(fast)
A certain reaction is second order in N2 and second order in H2 . Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. N2 H2 initial rate of reaction 1.18M 1.86M ×8.00105/Ms 0.579M 1.86M /Ms 0.398M 5.52M /Ms
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
Consider the mechanism. AB+C Step 1: Step 2: C + D E Overall: A+DB + E Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate= slow fast
b The half-life of a reaction, t1/2t1/2, is the time it takes for the reactant concentration [A][A] to decrease by half. For example, after one half-life the concentration falls from the initial concentration [A]0[A]0 to [A]0/2[A]0/2, after a second half-life to [A]0/4[A]0/4, after a third half-life to [A]0/8[A]0/8, and so on. on.
The data below were collected for the following reaction: CH3CI (g) + 3 Cl2 (g) → CCI4 (g) + 3 HCI (g) [CH3CI](M) [Cl2](M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.029 0.100 0.100 0.041 0.200 0.200 0.115 What is the order of the reaction with respect to CH3CI? What is the order of the reaction with respect to Cl2? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Write an expression for the reaction rate law.
A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g) → N₂(g) + H₂O(g) What is the rate law? More information is needed to answer this question. Or = K[H₂][NO] Or = K[H₂]²[NO]² Or = K[H₂][NO]² Or=K[H₂]²[NO] (slow) (fast)
Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88