[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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 36QRT

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Question

[RCOOH], M
[R’OH], M
[HA], M
Initial Rate, M•min¨
23.
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]
%3D
Rate = k[RCOOH][R'OH][HA]
Rate = k[RCOOR']/{[RCOOH][R'OH]}
%3D
Rate = k[R'OH]
Rate = k[RCOOH]
%D
Identify the rate-determining step based on the rate law you found
in question 23.
25.
0–H
ki
R-
С-0—Н
+ HA
R-¢+
A-
k2
0–H
Group 1
0–H
0–H
k3
R-C+
A-
R
-0–H
R—C—0—Н
k4
О—Н
R-ó+
A-
Group 2
H
0–H
R—С—0—н
k5
R+C-0–R'
+ H2O
+ HA
R-ó+
A-
Group 3
H.
Step 2 or Step 3
Step 1 or Step 2
Step 1 or Step 3
Step 2
Step 1
O Oo O O

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