Homework Help is Here – Start Your Trial Now!
Science
Chemistry
A student carres out the equilibrium constant experiment for the formation of FeSCN" (ag) using iron() nitrate and potassium thiocyanate folowing a simitar procedure used in the Virtual Labs simulator In this experiment, the absorbance values of solutions with anown product concentrations are measured to construct a Beer's Law plot Then, the absorbances of test moxtures are ottained to determine the unknown product concentration at equilibrium Fe"Cae) + SCN (ae)=FESCN" (ag) In the frst part of the lab, a student mistakenly uses 0.002M potassium thiocyanate solution to make the calibration solutions instead of 0.001 M potassum thiocyanate solution. The student moxes the test solutions using the correct concertrations If the student calculated the equilibrium concentrations of the ron(M) thiocyanate complex thinking the 0.001 M solution was used, what would the effect be on the student's resulta? Select the single best answer O The slope of the Beer's Law plot would be less than it should have been, resulting in smailer K, values calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in larger K, vatues calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in smaler K, values calculated in the second part of the experiment. O The slope of the Beer's Law plot would be less than it should have been, resulting in targer K, values calculated in the second part.

A student carres out the equilibrium constant experiment for the formation of FeSCN" (ag) using iron() nitrate and potassium thiocyanate folowing a simitar procedure used in the Virtual Labs simulator In this experiment, the absorbance values of solutions with anown product concentrations are measured to construct a Beer's Law plot Then, the absorbances of test moxtures are ottained to determine the unknown product concentration at equilibrium Fe"Cae) + SCN (ae)=FESCN" (ag) In the frst part of the lab, a student mistakenly uses 0.002M potassium thiocyanate solution to make the calibration solutions instead of 0.001 M potassum thiocyanate solution. The student moxes the test solutions using the correct concertrations If the student calculated the equilibrium concentrations of the ron(M) thiocyanate complex thinking the 0.001 M solution was used, what would the effect be on the student's resulta? Select the single best answer O The slope of the Beer's Law plot would be less than it should have been, resulting in smailer K, values calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in larger K, vatues calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in smaler K, values calculated in the second part of the experiment. O The slope of the Beer's Law plot would be less than it should have been, resulting in targer K, values calculated in the second part.

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
please explain
A student carres out the equilibrium constant experiment for the formation of FESCN" (ag) using iron() nitrate and potassium thiocyanate folowing a similar procedure used in the Virtual Labs simulator In this experiment, the absortbance values of solutions with known product cancentrations are measured to construct a Deer's Law plot Then, the absorbances of test moxtures are ottained to determine the unknown product toncentration at equilibrium. Fe"Caa) + SCN (ae)FESCN" (ag) In the first part of the lab, a student mistakenly uses 0.002 M potassium thiocyanate solution to make the calitration solutions instead of 0.001 M petassum thiocyanate solution, The student mixes the test solutions using the correct concertrations. If the student calculated the equilibrium concentrations of the Iron(M) thiocyanate complex thinking the 0.001 M solution was used, what would the effect be on the student's resulta? Select the single best answer O The slope of the Beer's Law plot would be less than it should have been, resulting in smaler K, values calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in larger K, values calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in smaler K, values calculated in the second part of the experiment. O The slope of the Beer's Law plot would be less than it should have been, resulting in larger K, values calculated in the second part.
Transcribed Image Text:A student carres out the equilibrium constant experiment for the formation of FESCN" (ag) using iron() nitrate and potassium thiocyanate folowing a similar procedure used in the Virtual Labs simulator In this experiment, the absortbance values of solutions with known product cancentrations are measured to construct a Deer's Law plot Then, the absorbances of test moxtures are ottained to determine the unknown product toncentration at equilibrium. Fe"Caa) + SCN (ae)FESCN" (ag) In the first part of the lab, a student mistakenly uses 0.002 M potassium thiocyanate solution to make the calitration solutions instead of 0.001 M petassum thiocyanate solution, The student mixes the test solutions using the correct concertrations. If the student calculated the equilibrium concentrations of the Iron(M) thiocyanate complex thinking the 0.001 M solution was used, what would the effect be on the student's resulta? Select the single best answer O The slope of the Beer's Law plot would be less than it should have been, resulting in smaler K, values calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in larger K, values calculated in the second part of the experiment. The slope of the Beer's Law plot would be greater than it should have been, resulting in smaler K, values calculated in the second part of the experiment. O The slope of the Beer's Law plot would be less than it should have been, resulting in larger K, values calculated in the second part.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Statistics and Analytical Chemistry
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.
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