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...
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Question
Using the images attached please write the produce in your own words
Please write it in a paragraph
Please answer as fast as possible
NOTE: Both images go together
Transcribed Image Text:I.
PROCEDURE
Solution Preparation.
Using burets OR volumetric pipets, prepare to measure out 0.01 M Fe(NO3)3
solution and 0.01 M H3SSA solution as listed below. Note the actual solution
concentrations as written on the dispensing containers. Make the following
solutions. All solutions must sit for 30 minutes before you measure their
absorbances, to give the chemicals time to come to equilibrium. You will
need to use solution G first; if you make it first, it can sit while you make the
other solutions.
![II.
III.
IV.
Volumes need NOT be exactly as listed, but you must know what they are to two places
after the decimal.
Determining max
The "blank" cuvette for the entire experiment should contain 0.100M HC1O4, NOT water.
Using solution G, find max. Range: 400-620nm in 20nm intervals. Near the highest A
value, take more data at 5nm intervals.
Solution Absorbances
(Refill your cuvette with fresh solution G.)
With the Genesis Spectrophotometer set at max, measure the absorbances of solutions
A-I. Then go back and measure all absorbances a second time.
Calculations and Results
A. Plot A vs λ for Solution G (A on the y axis, λ on the x axis.)
B. Beer's Law
C.
In solutions A-D, essentially all of the Fe³+ reacts to form FeSSA. There are two
reasons for this. First, the equilibrium constant for the formation of the product is
large. Secondly, adding excess H₂SSA forces the reaction to the right.
D.
Therefore, for each of these solutions you can calculate the final [FeSSA]. Plot
absorbance (on the y axis) vs concentration of FeSSA (on the x axis.) This
MUST be a computer graph with a computer fit, straight line through 0,0! Report
el with units. Find the slope of the straight line through these data points.
Determine Ke the equilibrium constant.
In this experiment, every solution you use contains 0.1M HClO4. This strong acid
is present to prevent chemical reactions that happen in less acidic environments.
Because the concentration of the strong acid never changes, the [H] is constant
and can be included in the equilibrium constant. Thus the equilibrium constant
we will determine is for the reaction:
Fe³+ (aq) + H₂SSA (aq) = FeSSA(aq) + (ignore the 2 H¹)
Using reaction tables and your data from solutions E-I, determine the equilibrium
constant independently for each solution E-I. Each solution will have a slightly
different reaction table and calculation. An example will be shown in class.
Calculate the average and relative range of the five resulting equilibrium
constants. Show ALL of your calculations either in your notebook or on separate
sheets, neatly!
Discussion/Conclusions. Summarize your results in a table showing the
equilibrium constants Kc that you calculated for each solution, as well as the average
and relative range. Comment on the precision. Should they all be the same? Why or
why not? Discuss why your experimental results may differ from theoretical
expections in this respect, ie, give an error analysis.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdab67aeb-c4d9-43f7-88d0-dfd6e7af2d5d%2Faf920bc7-6b4e-45db-a05f-df70eb5c78ab%2F0ajm8x_processed.jpeg&w=3840&q=75)
Transcribed Image Text:II.
III.
IV.
Volumes need NOT be exactly as listed, but you must know what they are to two places
after the decimal.
Determining max
The "blank" cuvette for the entire experiment should contain 0.100M HC1O4, NOT water.
Using solution G, find max. Range: 400-620nm in 20nm intervals. Near the highest A
value, take more data at 5nm intervals.
Solution Absorbances
(Refill your cuvette with fresh solution G.)
With the Genesis Spectrophotometer set at max, measure the absorbances of solutions
A-I. Then go back and measure all absorbances a second time.
Calculations and Results
A. Plot A vs λ for Solution G (A on the y axis, λ on the x axis.)
B. Beer's Law
C.
In solutions A-D, essentially all of the Fe³+ reacts to form FeSSA. There are two
reasons for this. First, the equilibrium constant for the formation of the product is
large. Secondly, adding excess H₂SSA forces the reaction to the right.
D.
Therefore, for each of these solutions you can calculate the final [FeSSA]. Plot
absorbance (on the y axis) vs concentration of FeSSA (on the x axis.) This
MUST be a computer graph with a computer fit, straight line through 0,0! Report
el with units. Find the slope of the straight line through these data points.
Determine Ke the equilibrium constant.
In this experiment, every solution you use contains 0.1M HClO4. This strong acid
is present to prevent chemical reactions that happen in less acidic environments.
Because the concentration of the strong acid never changes, the [H] is constant
and can be included in the equilibrium constant. Thus the equilibrium constant
we will determine is for the reaction:
Fe³+ (aq) + H₂SSA (aq) = FeSSA(aq) + (ignore the 2 H¹)
Using reaction tables and your data from solutions E-I, determine the equilibrium
constant independently for each solution E-I. Each solution will have a slightly
different reaction table and calculation. An example will be shown in class.
Calculate the average and relative range of the five resulting equilibrium
constants. Show ALL of your calculations either in your notebook or on separate
sheets, neatly!
Discussion/Conclusions. Summarize your results in a table showing the
equilibrium constants Kc that you calculated for each solution, as well as the average
and relative range. Comment on the precision. Should they all be the same? Why or
why not? Discuss why your experimental results may differ from theoretical
expections in this respect, ie, give an error analysis.
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