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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: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 11.ACP: (Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a...
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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
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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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 ?
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 ?
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