
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
![The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous
hydroxide solution:
OCI+I → OI+ CI
Experiment [OC]o, M [Ilo, M Initial Rate, M. s-¹
0.00135
0.00173
1.56 × 10-4
0.00135
0.00347
3.12 x 10-4
0.00271
0.00173
3.12 x 10-4
0.00271
0.00347 6.26 × 10-4
1
2
3
4
Complete the rate law for this reaction in the box below.
Use the form k[A] [B]", where '1' is understood for m or ʼn and concentrations taken to the zero
power do not appear. Don't enter 1 for m or n.
Rate =
k=
M-¹.s-¹](https://content.bartleby.com/qna-images/question/2a948ce4-bfec-4c4b-a693-d4721e6497c9/bcfdc051-d5a1-4cfa-b4a8-a61cfc93e7f7/x206fr_thumbnail.jpeg)
Transcribed Image Text:The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous
hydroxide solution:
OCI+I → OI+ CI
Experiment [OC]o, M [Ilo, M Initial Rate, M. s-¹
0.00135
0.00173
1.56 × 10-4
0.00135
0.00347
3.12 x 10-4
0.00271
0.00173
3.12 x 10-4
0.00271
0.00347 6.26 × 10-4
1
2
3
4
Complete the rate law for this reaction in the box below.
Use the form k[A] [B]", where '1' is understood for m or ʼn and concentrations taken to the zero
power do not appear. Don't enter 1 for m or n.
Rate =
k=
M-¹.s-¹
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 3 steps with 20 images

Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 23. The following data were measured for the reaction BF3(g) + NH3(g) ---> F3BNH3(g) Experiment [BF3] (M) [NH3] (M) initial rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 What is the overall order of the reaction? Group of answer choices A. 3 B. 2 C. 1 D. 0arrow_forwardConsider this reaction and the following data table for this reaction 2N 2O 5 -->4NO 2+ O 2 The following data table shows the decrease in N 2O 5 concentration with time at 25 oC. Time (s) concentration N 2O 5 , M 0.000 0.124 10.00 0.110 20.00 0.0880 30.00 0.0730 40.00 0.0540 Use the table to calculate the average rate of reaction between 10s and 30 s. Consider this reaction and the following data table for this reaction 2N 2O 5-->4NO 2+ O 2 The following data table shows the decrease in N 2O 5 concentration with time at 25 oC. Time (s) concentration N 2O 5 , M 0.000 0.124 10.00 0.110 20.00 0.0880 30.00 0.0730 40.00 0.0540 Use the table to calculate the…arrow_forwardExpress the average reaction rate for each time interval in moles of O2 produced per liter per minute. 0-100 s 500-600 s 1100-1200 sarrow_forward
- Can someone please help with question 5 b and carrow_forward5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.arrow_forwardConsider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.arrow_forward
- 3. The following results were obtained by monitoring the reaction + 1e+1/2 H,Oo) 1/2 I(a0)+ H,O (bo) rate l'o'Hl 0.020 0.020 3.3 x 105 0.040 0.020 6.6 x 105 0.020 9.0 x 10-5 0.040 0.040 1.3 x 104 Determine the order of the reaction with respect to I' and H,O, and also determine the value for the rate constant, karrow_forwardThe following data were collected for a certain reaction of the type A +B → products. Determine the specific rate constant for this reaction. [A]o, mol L-1 [B]o, mol L-1 Initial rate, mol L-1 s-1 Run i 0.200 0.300 2.44 x 10-2 ii 0.200 0.450 2.44 x 10-2 i 0.300 0.450 5.49 x 10-2 O A. 0.610 L mol s-1 B. 0.960 L mol1 s-1 C. 0.271 L mol-1 s-1 D. 0.407 L mol-1 s-1 O E. 0.120 L mol-1 s-1arrow_forwardDo not give handwriting solution.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY