**Question 8**The following questions are based on the reaction and data below.Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution, this reaction takes place:\[ 2 \text{ClO}_2 (\text{aq}) + 2 \text{OH}^- (\text{aq}) \rightarrow \text{ClO}_2^- (\text{aq}) + \text{ClO}_3^- (\text{aq}) + \text{H}_2\text{O}(\text{l}) \]Based on the following data, determine the rate law and the value of the rate constant.| Initial Concentrations | Initial Rate (M/s) ||------------------------|--------------------|| [ClO\(_2\)] = 0.060 M | [OH\(^-\)] = 0.030 M | 0.0248 || [ClO\(_2\)] = 0.020 M | [OH\(^-\)] = 0.030 M | 0.00276 || [ClO\(_2\)] = 0.020 M | [OH\(^-\)] = 0.090 M | 0.00828 |What is the order of the reaction with respect to ClO\(_2\)?- Fourth order- Zero order- Second order- First order---**Explanation:**To determine the reaction order with respect to each reactant, observe how changes in concentration affect the rate. For example:- Compare experiments where only one reactant concentration changes while the other remains constant.- Calculate the rate constant from the rate law once the orders are established.

Answered: Image /qna-images/answer/2b17be01-5872-4df2-8b34-4e83962821d2.jpg

Answered: The following questions are based on…

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

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0041 M-s 2NH₂(g) → N₂(g) + 3 H₂ (g) Suppose a 450. mL flask is charged under these conditions with 100. mmol of ammonia. After how much time is there only 50.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 X S
At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 3.35 s¯¹: NH,OH (aq) → NH, (aq)+H,O (aq) 4 Suppose a vessel contains NH4OH at a concentration of 0.260M. Calculate the concentration of NH4OH in the vessel 0.230 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M ■ x10 X
Consider this reaction: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) At a certain temperature it obeys this rate law. =(0.0152 s¹)[H₂CO3] rate = Suppose a vessel contains H₂CO3 at a concentration of 0.250M. Calculate the concentration of H₂CO3 in the vessel 56.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X
Consider the following fictitious balanced chemical equation below. In the first 315.0 seconds of the reaction, the concentration of B falls from 0.1597 M to 0.0672 M. What is the average rate of this reaction? 7 A (g) + 4 B (g) → 5 C (g) + 6 D (g)
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0044 M's : 2 HI (g) - H, (g) +I, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of hydrogen iodide. How much is left 8.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10
Consider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)
Consider the following fictitious balanced chemical equation below. In the first 230.0 seconds of the reaction, the concentration of B falls from 0.2836 M to 0.1626 M. What is the average rate of this reaction? 5 A (g) + 7 B (g) → 4 C (g) + 6 D (g)
The "iodine clock reaction" is a popular chemical demonstration. As part of that demonstration, the I3 ion is generated in the reaction S₂O3(aq) + 31¯(aq) → 2 SO²¯(aq) + 15 (aq) In one trial, the unique rate of reaction was 5.71 µmol·L¯ What was the rate of reaction of iodide ions? rate of reaction: What was the rate of formation of sulfate ions? rate of formation: •S μmol-L-¹.s-1 μmol-L-¹.s-1
I completed the problem but for some reason, my answer is still wrong. for part a I got 5.48 x 10^-5 and for part b I got 5.61x10^-4. I substituted the concentrations in the equation but hey still seem to be wrong can someone explain?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0045 M's : 2 HI (g) → H, (g)+I, (g) Suppose a 250. mL flask is charged under these conditions with 350. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10
The following reaction was studied at 25°C. The following results were obtained. a) What is the rate law for this reaction at this temperature? b) What is the value of the rate constant? Be sure to include the correct units in your answer.

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

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

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

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

SEE MORE TEXTBOOKS