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.
Chapter23: Voltammetry
Section: Chapter Questions
Problem 23.13QAP
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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.
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