Question 23Identify the rate-determining step based on the rate law you foundin question 23.Given these data for the acid-catalyzed reaction in question 22, fındthe rate law.0–H[RCOOH], M[R'OH], M(HA], MInitial Rate, Ml·min'||R-c-o–H0.350.350.504.600.50+ HA- R-Ć+k20.620.358.14A-0.350.810.5010.60.350.500.759.840–HGroup 1Rate = k[RCOOH][R'OH]0–H0–Hk3O Rate = k[RCOOH][R'OH][HA]R-C+A + R-0–HR—С—0—НRate = k[RCOOR']/{[RCOOH][R'OH]}k40–HR'-o+A-Rate = k[R'OH]Group 2HRate = k[RCOOH]0–Hk5R—С—0—нR-C-0–R'+ H2O+ HAR-o+A-Group 3H.Step 2 or Step 3Step 1 or Step 2Step 1 or Step 3Step 2Step 1

Determination of rate law: Rate=kRCOOHaR'OHbHAc Substituting the values: 1)…

Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOHL, M (R'OHL M (HAJ, M Initial Rate, M-min" ki 0.35 0.35 0.50 4.60 0.62 0.35 0.50 8.14 R- -С-0—н + HA R-C+ A- 0.35 081 0.50 10.6 0.35 0.50 0.75 9.84 k2 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A- + R -0–H R—С—0—н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R-ó+ A- Rate = k[R'OH] Group 2 H O Rate = k[RCOOH] 0–H ks R-C–0–R' + H2O + HA R–C–0-H R'-o+ A- Group 3 H Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 O Step 1 oooo

Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOHL, M (R'OHL M (HAJ, M Initial Rate, M-min" ki 0.35 0.35 0.50 4.60 0.62 0.35 0.50 8.14 R- -С-0—н + HA R-C+ A- 0.35 081 0.50 10.6 0.35 0.50 0.75 9.84 k2 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A- + R -0–H R—С—0—н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R-ó+ A- Rate = k[R'OH] Group 2 H O Rate = k[RCOOH] 0–H ks R-C–0–R' + H2O + HA R–C–0-H R'-o+ A- Group 3 H Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 O Step 1 oooo

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...

See similar textbooks

Similar questions

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
he reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0359 0.0359 0.0209 2 0.0359 0.0718 0.0418 3 0.0718 0.0359 0.0837 4 0.0718 0.0718 0.167 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate = k [ClO2(aq)]4 [OH-(aq)] (b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of ClO2(aq) is 0.0640 M and that of OH-(aq) is 0.0732 M if the temperature is the same as that used to obtain the data shown above? M/s
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] N2 H2 initial rate of reaction 1.27M 0.589М 22.0M/s 1.27 M |0.149 М 5.57 M/s 0.445 M 0.589M 2.70M/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 |I| х10 k =
Determine the (a) rate law (b) solve for the order, and (c) value of rate constant for the reaction. C + D + E ⟶⟶ Products Reaction # [C]0 [D]0 [E]0 Initial rate (mol/L s) 1 0.400 0.300 0.560 7.14 x 10 -4 2 0.100 0.500 0.200 4.55 x 10 -5 3 0.100 0.200 0.200 4.55 x 10 -5 4 0.400 0.300 0.750 1.28 x 10 -3 5 0.100 0.300 0.560 3.57 x 10 -4
7 11 The initial rate of the reaction has been measured at the reactant concentrations show: Trial [BrO3] [H*] (mol/L) (mol/L) 0.10 0.10 0.20 0.10 0.10 0.20 0.10 0.10 1 23 3. 4 The rate law expression will be: [Br] (mol/L) 0.10 0.10 0.10 0.20 Initial rate (mol/L.s) 8.0 16 16 32
or a reaction involving two reagents A and B, the following data was collected over three experiments. Exp# [A] [B] Rate (M/s) 1 0.20 M 0.20 M 5.0 2 0.20 M 0.40 M 20.0 3 0.10 M 0.40 M 10.0 Using the above data, which of the following is the rate law for the reaction of A with B?
Solve it asap
The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is