Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The data shown below are Fe(II) concentrations observed at two different depths over an incubation period. They illustrate Fe(II) oxidation in the sediments that were incubated. Time (d) Fe(II) (mM) 0 cm Fe(II) (mM) 45 cm 0.00 13.63 7.39 4.00 2.71 8.04 7.00 0.40 6.97 11.00 0.05 3.93 14.00 0.37 1.66 21.00 0.43 0.59 28.00 0.28 0.37 a) Please calculate the first-order rate constants for Fe(II) oxidation at those two depths. g) please provide the half life for dissolved Fe(II).

The data shown below are Fe(II) concentrations observed at two different depths over an incubation period. They illustrate Fe(II) oxidation in the sediments that were incubated. Time (d) Fe(II) (mM) 0 cm Fe(II) (mM) 45 cm 0.00 13.63 7.39 4.00 2.71 8.04 7.00 0.40 6.97 11.00 0.05 3.93 14.00 0.37 1.66 21.00 0.43 0.59 28.00 0.28 0.37 a) Please calculate the first-order rate constants for Fe(II) oxidation at those two depths. g) please provide the half life for dissolved Fe(II).

Chemistry
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
icon
Related questions
Question

The data shown below are Fe(II) concentrations observed at two different depths over an incubation period.  They illustrate Fe(II) oxidation in the sediments that were incubated.

Time (d)

Fe(II) (mM) 0 cm

Fe(II) (mM) 45 cm

0.00

13.63

7.39

4.00

2.71

8.04

7.00

0.40

6.97

11.00

0.05

3.93

14.00

0.37

1.66

21.00

0.43

0.59

28.00

0.28

0.37

 

  • a) Please calculate the first-order rate constants for Fe(II) oxidation at those two depths.
  • g) please provide the half life for dissolved Fe(II).
The data shown below are Fe(II) concentrations observed at two different depths over an incubation period. They illustrate Fe(II) oxidation in the sediments that were incubated. | Time (d) | Fe(II) (mM) 0 cm | Fe(II) (mM) 45 cm | |----------|------------------|-------------------| | 0.00 | 13.63 | 7.39 | | 4.00 | 2.71 | 8.04 | | 7.00 | 0.40 | 6.97 | | 11.00 | 0.05 | 3.93 | | 14.00 | 0.37 | 1.66 | | 21.00 | 0.43 | 0.59 | | 28.00 | 0.28 | 0.37 | a) Please calculate the first-order rate constants for Fe(II) oxidation at those two depths. g) Please provide the half-life for dissolved Fe(II).
Transcribed Image Text:The data shown below are Fe(II) concentrations observed at two different depths over an incubation period. They illustrate Fe(II) oxidation in the sediments that were incubated. | Time (d) | Fe(II) (mM) 0 cm | Fe(II) (mM) 45 cm | |----------|------------------|-------------------| | 0.00 | 13.63 | 7.39 | | 4.00 | 2.71 | 8.04 | | 7.00 | 0.40 | 6.97 | | 11.00 | 0.05 | 3.93 | | 14.00 | 0.37 | 1.66 | | 21.00 | 0.43 | 0.59 | | 28.00 | 0.28 | 0.37 | a) Please calculate the first-order rate constants for Fe(II) oxidation at those two depths. g) Please provide the half-life for dissolved Fe(II).
Expert Solution
Step 1

NOTE : The data looks to be somewhat incorrect. The value of concentration should be decreasing with time and not increasing. But in data there are points where the concentration is increasing.

Since we know that the relationship between the concentration of reactant i.e [A] and time for a first order process is given by 

Chemistry homework question answer, step 1, image 1

where [A] = final concentration of reactant

[A]0 = initial concentration of reactant 

t = time 

K = Rate constant 

steps

Step by step

Solved in 3 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Rate Laws
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
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS