3. The decomposition of a herbicide A in a water at 20° C is a 1st-order reaction with half-life of 2.0 months. Whatis a rate constant for this reaction? How long it will take for the concentration of herbicide to decrease from1.6*106 M to 1*107 M?

Given:Half-life = 2 months.Initial concentration No = 1.6×10-6 MFinal concentration N = 1×10-7 M

Answered: 3. The decomposition of a herbicide A…

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

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. = (0.291 M¹s¹) [N₂0₂] rate Suppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Subm Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente 80°F Partly sunny ^ pe here to search B X G
The half-life of a pesticide determines its persistence in the environment. A common pesticide degrades in a first-order process with a half-life of 6 days. What fraction (in decimal notation) of the pesticide remains in the environment after 20 days? Enter to 4 decimal places.
-1. Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0058 M-s: 2N₂O(g) → 2N₂ (g) +0₂ (8) Suppose a 2.0 L flask is charged under these conditions with 450. mmol of dinitrogen monoxide. After how much time is there only 225. 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 S Ala X 2. ?
A particular reactant decomposes with a half-life of 173 s when its initial concentration is 0.301 M. The same reactant decomposes with a half-life of 231 s when its initial concentration is 0.225 M. Determine the reaction order. 01 0 2 What is the value and units of the rate constant for this reaction? k = Units
The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.14 M, what is its concentration after exactly 7 minutes have passed?
The rate constant for a first order reaction is 0.54 s-1. If a 1.57 M sample reacts for 12 seconds, what concentration (in molarity) will remain?
The reactant concentration in a second-order reaction was 0.230 M after 230 s and 4.20×10−2 M after 725 s . What is the rate constant for this reaction?
The decomposition of aqueous hydrogen peroxide (H2O2) to gaseous oxygen and water is a 1st order process. If it takes 6.0 h for the concentration of H2O2 to decrease from 0.40 M to 0.20 M, how many hours are required for the concentration to decrease from 0.70 M to 0.35 M?
Cc.59.
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0039 M²s¯¹: 2N₂O(g) 2 N₂(g) + O₂(g) Suppose a 4.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. How much is left 6.0 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. 0 00 X 3
Solve it asap
A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻ because it is first order for I - . After you find the reaction order for S2O82⁻ you need to calculate k. S2O82⁻ (aq) + 3 I⁻ (aq) → 2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 ) 0.30 0.42 4.54 0.44 0.42 6.65 Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] Rate = 195 M-3s-1 [S2O82⁻]2[I⁻] Rate = 86 M-2s-1 [S2O82⁻][I⁻] Rate = 23 M-1/2s-1 [S2O82⁻][I⁻] Rate = 36 M-1s-1 [S2O82⁻][I⁻]

SEE MORE QUESTIONS

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

3. The decomposition of a herbicide A in a water at 20° C is a 1st-order reaction with half-life of 2.0 months. What is a rate constant for this reaction? How long it will take for the concentration of herbicide to decrease from 1.6*106 M to 1*107 M?

3. The decomposition of a herbicide A in a water at 20° C is a 1st-order reaction with half-life of 2.0 months. What is a rate constant for this reaction? How long it will take for the concentration of herbicide to decrease from 1.6106 M to 1107 M?