[RCOOH], M[R’OH], M[HA], MInitial Rate, M•min¨23.0.350.350.504.600.620.350.508.140.350.810.5010.60.350.500.759,84Rate = k[RCOOH][R'OH]%3DRate = k[RCOOH][R'OH][HA]Rate = k[RCOOR']/{[RCOOH][R'OH]}%3DRate = k[R'OH]Rate = k[RCOOH]%DIdentify the rate-determining step based on the rate law you foundin question 23.25.0–HkiR-С-0—Н+ HAR-¢+A-k20–HGroup 10–H0–Hk3R-C+A-R-0–HR—C—0—Нk4О—НR-ó+A-Group 2H0–HR—С—0—нk5R+C-0–R'+ H2O+ HAR-ó+A-Group 3H.Step 2 or Step 3Step 1 or Step 2Step 1 or Step 3Step 2Step 1O Oo O O

Here we have to apply the rate law Rate law=k[RCOOH]a[R'OH]b[HA]c

[RCOOH], M [R’OH], M (HA], M Initial Rate, M-min¨ 0.35 0.35 0.50 4.60 0.62 0.35 0.50 8.14 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 Rate = k[RCOOH][R'OH] Rate = k[RCOOH][R'OH][HA] %3D Rate = k[RCOOR']/{[RCOOH][R'OH]} Rate = k[R'OH] Rate = k[RCOOH] %3D

[RCOOH], M [R’OH], M (HA], M Initial Rate, M-min¨ 0.35 0.35 0.50 4.60 0.62 0.35 0.50 8.14 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 Rate = k[RCOOH][R'OH] Rate = k[RCOOH][R'OH][HA] %3D Rate = k[RCOOR']/{[RCOOH][R'OH]} Rate = k[R'OH] Rate = k[RCOOH] %3D

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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