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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

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

Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.59P
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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 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,
Transcribed Image Text: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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