Chem 125 Lab 8

.docx

School

University of Michigan**We aren't endorsed by this school

Course

CHEM 125

Subject

Statistics

Date

Jan 15, 2025

Pages

Uploaded by MasterIce2499

Lab 8 WorksheetTable 1. Raw Data (5pts)Trial[I–][BrO3–][H+]Time (sec)Relative rate value (reactions per sec.)10.002 M0.008 M 0.02 M144.831000/144.83 = 6.904620.002 M0.016 M0.02 M73.331000/73.33 = 13.6430.002 M0.008 M0.04 M35.821000/35.82 = 27.9240.004 M0.008 M0.02 M67.561000/67.56 = 14.8050.0016 M0.004 M0.03 M168.221000/168.22 = 5.9446Questions:1.Calculate m for the rate law. Which two trials did you compare? (3pts)Trial 4/Trial 1 14.80/6.9046 = kI[0.004]m[0.008]n[0.02]p/kI[0.002]m[0.008]n[0.02]p2.144 = 2mlog10 (2m) = log10 (2.144)mlog10 (2) = log10 (2.144)m = log10 (2.144)/log10 (2)m = 1.072m = 12.Calculate n for the rate law. Which two trials did you compare? (3pts)Trial 2/Trial 1 13.64/6.9046 = kI[0.002]m[0.016]n[0.02]p/kI[0.002]m[0.008]n[0.02]p1.975 = 2nlog10 (2n) = log10 (1.975)nlog10 (2) = log10 (1.975)n = log10 (1.975)/log10 (2)n = 0.9875n = 1

3.Calculate p for the rate law. Which two trials did you compare? (3pts)Trial 3/Trial 1 27.92/6.9046 = kI[0.002]m[0.008]n[0.04]p/kI[0.002]m[0.008]n[0.02]p4.043 = 2plog10 (2p) = log10 (4.043)plog10 (2) = log10 (4.043)p = log10 (4.043)/log10 (2)p = 2.022p = 2Table 2. k’ values (2pts) Show an example of how you solved ONE belowSolution 1Solution 2Solution 3Solution 4Solution 5k'1.732 x 1091.725 x 1091.724 x 1091.766 x 1091.654 x 109Average k’1.720 x 109Standard deviation+1Trial 1 = kI[0.002]m[0.008]n[0.02]p6.9046 = kI[0.002]1[0.008]1[0.02]26.9046/(3.987 x 10-9)kIkI= 1.732 x 1094.What is the complete relative rate law equation you found in this lab? (use your average k’) (2pts)Relative Rate = kI[A]m[B]n[C]pRelative Rate = (1.720 x 109)[I–]m[BrO3–]n[H+]pRelative Rate= (1.720 x 109)[I–]1[BrO3–]1[H+]25.What does the rate law tell you about this reaction? What compound is the reaction most dependent upon? (2pts)The rate law demonstrates the relationship between the concentration of reactants in a chemical reaction and the rate at which the reaction occurs. Analyzing the rate law above, it is clear that reactants with a higher order will affect the reaction rate to a higher degree than those with lower orders. Subsequently, the rate of this reaction is most dependent on hydrochloric acid (HCl), which has an order of two, twice the order of both other reactants.