By what factor does increasing the temperature of a reaction from T₁ = 289 K to T₂ = 299 K increase the rate of reaction? Assume the activation energy (Ea) of this reaction is 164,500 J and that the pre-exponential constant (A) is 2.1 x 10⁹ s-¹. Express your answer to one decimal place. k₂/k1 = 17| ΑΣΦ ?
By what factor does increasing the temperature of a reaction from T₁ = 289 K to T₂ = 299 K increase the rate of reaction? Assume the activation energy (Ea) of this reaction is 164,500 J and that the pre-exponential constant (A) is 2.1 x 10⁹ s-¹. Express your answer to one decimal place. k₂/k1 = 17| ΑΣΦ ?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.99PAE: Substances that poison a catalyst pose a major concern for many engineering designs, including those...
Related questions
Question
8L.13.1
![providing a lower energy pathway between the reactants and the products. This usually involves the formation of a transition state or an intermediate that cannot be
formed without the catalyst. The catalyzed reaction pathway generally has a much lower activation energy barrier than is required for the direct reaction of reactants to
products. Notice what catalysts do not do: They do not change the energy of the reactants, products, or overall reaction. What changes is the activation energy.
Part A
k₂/k1
=
Eact
No catalvat
Submit
Energy Reactants
——| ΑΣΦ
The collision theory of reactions states that, for a reaction to occur, molecules must collide with sufficient energy and the proper orientation. A catalyst can increase the
rate of reaction by increasing the probability of the molecules colliding with the correct orientation. Increasing the temperature can also increase the rate of a reaction,
as it increases both the energy of the molecules and the number of collisions between molecules.
Request Answer
No catalyst
=
The connection among the rate of the reaction, temperature, and activation energy is given by the Arrhenius equation: k Ae-Ea/RT, where k is the rate constant for
the reaction rate, Ea is the activation energy, R is the gas constant, equal to 8.314 J/(mol · K), T is the temperature in kelvins, and A is the pre-exponential
constant for the reaction. The pre-exponential constant has the same units as k.
With catalyst
Eact
+ catalyst
By what factor does increasing the temperature of a reaction from T₁ = 289 K to T₂ = 299 K increase the rate of reaction? Assume the activation energy (Ea) of
this reaction is 164,500 J and that the pre-exponential constant (A) is 2.1 × 10⁰⁹ s-¹.
Express your answer to one decimal place.
?
Progress of reaction →
LAH₂
Products](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F52db8ee6-33d1-4aac-bbe4-ebc771de1e49%2F29848bc9-f7c7-4470-a460-df8261bd85f2%2Fd4kieb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:providing a lower energy pathway between the reactants and the products. This usually involves the formation of a transition state or an intermediate that cannot be
formed without the catalyst. The catalyzed reaction pathway generally has a much lower activation energy barrier than is required for the direct reaction of reactants to
products. Notice what catalysts do not do: They do not change the energy of the reactants, products, or overall reaction. What changes is the activation energy.
Part A
k₂/k1
=
Eact
No catalvat
Submit
Energy Reactants
——| ΑΣΦ
The collision theory of reactions states that, for a reaction to occur, molecules must collide with sufficient energy and the proper orientation. A catalyst can increase the
rate of reaction by increasing the probability of the molecules colliding with the correct orientation. Increasing the temperature can also increase the rate of a reaction,
as it increases both the energy of the molecules and the number of collisions between molecules.
Request Answer
No catalyst
=
The connection among the rate of the reaction, temperature, and activation energy is given by the Arrhenius equation: k Ae-Ea/RT, where k is the rate constant for
the reaction rate, Ea is the activation energy, R is the gas constant, equal to 8.314 J/(mol · K), T is the temperature in kelvins, and A is the pre-exponential
constant for the reaction. The pre-exponential constant has the same units as k.
With catalyst
Eact
+ catalyst
By what factor does increasing the temperature of a reaction from T₁ = 289 K to T₂ = 299 K increase the rate of reaction? Assume the activation energy (Ea) of
this reaction is 164,500 J and that the pre-exponential constant (A) is 2.1 × 10⁰⁹ s-¹.
Express your answer to one decimal place.
?
Progress of reaction →
LAH₂
Products
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Follow-up Question
8L.13.3
![The rate of an enzyme-catalyzed reaction is 2.26×105 times faster than the rate of the uncatalyzed reaction. What is the difference in Ea between the uncatalyzed
and catalyzed reactions at T = 262K ?
Express your answer with the appropriate units.
μA
Value
Units
?](https://content.bartleby.com/qna-images/question/52db8ee6-33d1-4aac-bbe4-ebc771de1e49/4cd51874-bcea-4c6a-8557-aceeca7cacf2/mumeqnx_thumbnail.jpeg)
Transcribed Image Text:The rate of an enzyme-catalyzed reaction is 2.26×105 times faster than the rate of the uncatalyzed reaction. What is the difference in Ea between the uncatalyzed
and catalyzed reactions at T = 262K ?
Express your answer with the appropriate units.
μA
Value
Units
?
Solution
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