Answered: By what factor does increasing the…

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

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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$**Reaction Dynamics and Catalysis** For a reaction to occur, bonds must be broken and/or made. This process includes a high-energy transition state. Formation of this transition state is energetically unfavorable. The difference in energy between the reactants and the transition state is called the activation energy. Catalysts can accelerate the chemical reaction by 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. **Diagram Explanation:** The diagram illustrates the energy profile of a reaction. There are two curves representing the reaction progress with and without a catalyst. The vertical axis represents energy, while the horizontal axis shows the progress of the reaction. - **Without Catalyst (No Catalyst):** The energy curve shows a high peak, indicating a higher activation energy (Ea) that reactants need to overcome to form products. - **With Catalyst:** The energy curve with a catalyst is lower, showing how the catalyst lowers the activation energy (Eₐ^catalyst). **Collision Theory of Reactions** 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. The connection among the rate of the reaction, temperature, and activation energy is given by the Arrhenius equation: $ k = A e^{-\frac{E_a}{RT}} $, where $ k $ is the rate constant for the reaction rate, $ E_a $ 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 $. **Part A** By what factor does increasing the temperature of a reaction from \( T_1 = 273 \$

Transcribed Image Text:**Reaction Dynamics and Catalysis** For a reaction to occur, bonds must be broken and/or made. This process includes a high-energy transition state. Formation of this transition state is energetically unfavorable. The difference in energy between the reactants and the transition state is called the activation energy. Catalysts can accelerate the chemical reaction by 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. **Diagram Explanation:** The diagram illustrates the energy profile of a reaction. There are two curves representing the reaction progress with and without a catalyst. The vertical axis represents energy, while the horizontal axis shows the progress of the reaction. - **Without Catalyst (No Catalyst):** The energy curve shows a high peak, indicating a higher activation energy (Ea) that reactants need to overcome to form products. - **With Catalyst:** The energy curve with a catalyst is lower, showing how the catalyst lowers the activation energy (Eₐ^catalyst). **Collision Theory of Reactions** 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. The connection among the rate of the reaction, temperature, and activation energy is given by the Arrhenius equation: $ k = A e^{-\frac{E_a}{RT}} $, where $ k $ is the rate constant for the reaction rate, $ E_a $ 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 $. **Part A** By what factor does increasing the temperature of a reaction from \( T_1 = 273 \

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