10. Consider the general form of a first order decomposition reaction. A + B with d[4] k,[A] dt a) If the rate constant obeys the Arrhenius equation with prefactor A=1012s-1, what is an upper bound on the activation energy Ea if a solution with [A]=1M is to react with initial rate of at least 10-3 M*s- at 298 K? b) If the activation energy is E, = 75 kJ/mol, how much would you have to increase the temperature in order to double this initial rate? c) From transition state theory, explain how you would know whether the change in entropy of forming the transition state ASt is positive or negative, based on the Arrhenius prefactor.
10. Consider the general form of a first order decomposition reaction. A + B with d[4] k,[A] dt a) If the rate constant obeys the Arrhenius equation with prefactor A=1012s-1, what is an upper bound on the activation energy Ea if a solution with [A]=1M is to react with initial rate of at least 10-3 M*s- at 298 K? b) If the activation energy is E, = 75 kJ/mol, how much would you have to increase the temperature in order to double this initial rate? c) From transition state theory, explain how you would know whether the change in entropy of forming the transition state ASt is positive or negative, based on the Arrhenius prefactor.
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Chapter1: Chemical Foundations
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Need a b c
![10. Consider the general form of a first order decomposition reaction.
A + B
with
d[A]
= k,[A]
dt
a) If the rate constant obeys the Arrhenius equation with prefactor A=1012s-1, what
is an upper bound on the activation energy Ea if a solution with [A]=1M is to react with
initial rate of at least 10-3 M*s- at 298 K?
b) If the activation energy is Ea = 75 kJ/mol, how much would you have to increase
the temperature in order to double this initial rate?
c) From transition state theory, explain how you would know whether the change in
entropy of forming the transition state ASt is positive or negative, based on the Arrhenius
prefactor.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F744af276-3b7c-49cb-a92c-d6b2708fe35d%2Fcdec9eb2-21c5-4d7e-837f-98426fe9db60%2Fvct9nqq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:10. Consider the general form of a first order decomposition reaction.
A + B
with
d[A]
= k,[A]
dt
a) If the rate constant obeys the Arrhenius equation with prefactor A=1012s-1, what
is an upper bound on the activation energy Ea if a solution with [A]=1M is to react with
initial rate of at least 10-3 M*s- at 298 K?
b) If the activation energy is Ea = 75 kJ/mol, how much would you have to increase
the temperature in order to double this initial rate?
c) From transition state theory, explain how you would know whether the change in
entropy of forming the transition state ASt is positive or negative, based on the Arrhenius
prefactor.
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