Note that our data is ABSORBANCE versus time, not CONCENTRATION versus time. Absorbance and concentration are proportional according to Beer's law A = abc or A = ElC so the data is still useful. However, extracting the rate constant from a linear plot may be annoying if the rate constant is supposed to incorporate units of concentration. For example, if the rate constant should be 0.25/s then there is no problem, but if the rate constant should be 0.25 M/s then how can we get the molar unit directly from a graph involving ABSORBANCE and time? We can't. We'd need to involve Beer's law. Hopefully we won't need to do that. Identify the symbols used in Beer's law. A molar absorbtivity/ extinction coefficient a molar concentration b absorbance path length through the sample с

Note that our data is ABSORBANCE versus time, not CONCENTRATION versus time. Absorbance and concentration are proportional according to Beer's law A = abc or A = ElC so the data is still useful. However, extracting the rate constant from a linear plot may be annoying if the rate constant is supposed to incorporate units of concentration. For example, if the rate constant should be 0.25/s then there is no problem, but if the rate constant should be 0.25 M/s then how can we get the molar unit directly from a graph involving ABSORBANCE and time? We can't. We'd need to involve Beer's law. Hopefully we won't need to do that. Identify the symbols used in Beer's law. A molar absorbtivity/ extinction coefficient a molar concentration b absorbance path length through the sample с

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

1. Consider the Following rate law: Rate= K[A] [BJ™ How are the exponents in and m determined ? a. A First-order redetion is 45 % Complete at the end of 35 minutes - What is the length of the half-life of this reaction?
An irreversible unimolecular reaction (A -> B) has a rate constant of 3.0 per second. What is the half-time (t1/2)? Type in your answer. t1/2 =
The raw data is plotted in figure A. Then I transformed the absorbance data to make figures B and C. A line (instead of a curve) on each plot would predict what reaction order for the rate law?
For a molecule, the phosphorescence lifetime without quenching is 1.0 s while with a quencher population of 10-2 M the phosphorescence lifetime is 0.10 s. Calculate the rate constant for phosphorescence assuming that kisc >> (kF + kec + kic). Calculate the rate constant for external conversion of the triplet state (kec’), the quenching rate constant for the triplet state (kq’), and the Stern-Volmer quenching constant. Assume that intersystem crossing from T1 to So is negligible.
I am taking an online chem class and it’s harder than I thought. I have the answers to my whole study guide but I want to understand the WHY of the answers. Thank you!
10
how do you calculate the rate constant, k, by using the orders, a, b, and c, that you calculated above, the rate and concentration data from Trial 1. Remember that a rate constant must have units. Write the full rate law for the reaction below including all the numbers you just calculated.
2. The physical mechanism involved in elementary reactions was given as: A+ A k1 A* + A activation by binary collisions A* + A A + A deactivation by binary collisions k2 A* + bA *, products reaction step where b = 0 for unimolecular reaction steps b = 1 for bimolecular reaction steps b = 2 for termolecular reaction steps. Carry out a steady state analysis to show that unimolecular reactions are first order at high pressures, moving to second order at low pressures. State the rate determining steps in each region. In contrast, show that bimolecular reactions are second order at all pressures.
1
please don't provide handwrittin solution....
Explain the transitions occurring when acetaldehyde (CH3-CHO) is exposed to EM radiation.
Living chain polymerization of monomer X follows the first-order kinetics. The corresponding propagation rate constant (kp) was determined by gas chromatography (GC), with the following monomer concentrations measured at different polymerization times, assuming instant initiation: Polymerization time (min) 0 2 5 10 15 [X]t (M) 1.80 1.52 1.27 0.95 0.74 0.50 0.25 20 30 Plot the dependence of -In([X]/[X]) on time using software specialized for graphs (e.g., Origin, SigmaPlot, not MS Excell!) and perform the linear data fitting. Export the graph in TIFF format and paste it below as an image. Make sure the graph is graphically appealing! b) From this fitting, calculate the kp of polymerization, assuming the living character of polymerization and an initial initiator concentration (an thus the constant concentration of growing centers) of 0.09 M c) What is the theoretical degree of polymerization (DP) of the prepared polymer? We assume full monomer conversion, complete initiation, absence of…