Based on the following data for thefırst order reaction Jproducts, calculatethe rate constant k (in s1).Time[J]Os1.0000 M900.52313000.1153O 2.9 x 104O 1.4 x 103O 5.3 x 10-4О 1.0 х 10-3O 7.2 x 10-4 R = .008314 kJ/K (Gas Constant)F = 96.485 kJ/(V mol)[A]pK, + log(班)[base]pHpK, + logORpH%3D[acid][HA]AG°AH° - TASºAG = AG° + RTINQAG° = -RT/nKeqAG° = -nFE°cell%3D0591EcellE°clllogQFirst OrderRadioactivitySecond Order[AloInXo1ktIn= kt= kt +[A]t[A][A]o.693.693ty =ty =ty =kkK[A]

We will use intergrated rate law for first order reaction to calculate rate constant.

Based on the following data for the fırst order reaction J products, calculate the rate constant k (in s-1). Time [J] Os 1.0000 M 900 .5231 3000 .1153 O 2.9 x 10-4 Ο 1.4 x 103 O 5.3 x 10-4 O 1.0 x 10-3 O 7.2 x 10-4

Based on the following data for the fırst order reaction J products, calculate the rate constant k (in s-1). Time [J] Os 1.0000 M 900 .5231 3000 .1153 O 2.9 x 10-4 Ο 1.4 x 103 O 5.3 x 10-4 O 1.0 x 10-3 O 7.2 x 10-4

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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Question

100%

Based on the following data for the
fırst order reaction J
products, calculate
the rate constant k (in s1).
Time
[J]
Os
1.0000 M
900
.5231
3000
.1153
O 2.9 x 104
O 1.4 x 103
O 5.3 x 10-4
О 1.0 х 10-3
O 7.2 x 10-4

R = .008314 kJ/K (Gas Constant)
F = 96.485 kJ/(V mol)
[A]
pK, + log
(班)
[base]
pH
pK, + log
OR
pH
%3D
[acid]
[HA]
AG°
AH° - TASº
AG = AG° + RTINQ
AG° = -RT/nKeq
AG° = -nFE°cell
%3D
0591
Ecell
E°cll
logQ
First Order
Radioactivity
Second Order
[Alo
In
Xo
1
kt
In
= kt
= kt +
[A]t
[A]
[A]o
.693
.693
ty =
ty =
ty =
k
k
K[A]

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