If the activation energy for a reaction is 60.6 kJ/mole, how many times faster is the reaction at 500 K than300 K?4306.1O 1.7x104O 9.7Thermodynamic relationships:T(K) = T(°C) + 273.15AG = AH - TASAG = -RT In(K)R=0.008314 kJ/(mol·K)%3D(-AHRTAS )K = eRKinetic relationships:Integrated rate laws:zero order: [C):= [C]o-kt first order: In[C] = In[C]o-ktsecond order: 1/[C]. =1/[C]o+ktE.E1kT..Е, 1+ In( A)R TRT2k = AeRTIn( k) =a.= e%3Dk T,

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If the activation energy for a reaction is 60.6 kJ/mole, how many times faster is the reaction at 500 K than 300 K? 430 O 6.1 O 1.7×10* O 9.7

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

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Question

100%

If the activation energy for a reaction is 60.6 kJ/mole, how many times faster is the reaction at 500 K than
300 K?
430
6.1
O 1.7x104
O 9.7
Thermodynamic relationships:
T(K) = T(°C) + 273.15
AG = AH - TAS
AG = -RT In(K)
R=0.008314 kJ/(mol·K)
%3D
(-AH
RT
AS )
K = e
R
Kinetic relationships:
Integrated rate laws:
zero order: [C):= [C]o-kt first order: In[C] = In[C]o-kt
second order: 1/[C]. =1/[C]o+kt
E.
E
1
kT..
Е, 1
+ In( A)
R T
RT2
k = Ae
RT
In( k) =
a.
= e
%3D
k T,

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