Answered: In the provided reaction profile, 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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$**Question 3 of 18** **Graph Explanation:** The graph illustrates the potential energy changes throughout a chemical reaction. It is labeled by "Potential Energy" on the vertical axis and "Reaction Progress" on the horizontal axis. The graph is divided into two main curves: one in black and another in red. - The black curve represents the energy profile without any catalyst, showing a high peak indicating a higher activation energy. - The red curve represents the reaction pathway in the presence of a catalyst, which presents a lower peak than the black curve, indicating reduced activation energy. The graph includes marked stages: - Initial state: $ \text{K + A + B} $ - Transition state (without catalyst): $ \text{K--A + B} $ - Transition state (with catalyst): $ \text{A--K--B} $ - Final products: $ \text{AB + K} $ **Multiple Choice Options:** A) Lowering the enthalpy of the reaction B) Lowering the activation energy of the reaction C) Changing the mechanism of the reaction D) Both A and B E) Both B and C *Reminder: Tap here or pull up for additional resources.*$

Transcribed Image Text:**Question 3 of 18** **Graph Explanation:** The graph illustrates the potential energy changes throughout a chemical reaction. It is labeled by "Potential Energy" on the vertical axis and "Reaction Progress" on the horizontal axis. The graph is divided into two main curves: one in black and another in red. - The black curve represents the energy profile without any catalyst, showing a high peak indicating a higher activation energy. - The red curve represents the reaction pathway in the presence of a catalyst, which presents a lower peak than the black curve, indicating reduced activation energy. The graph includes marked stages: - Initial state: $ \text{K + A + B} $ - Transition state (without catalyst): $ \text{K--A + B} $ - Transition state (with catalyst): $ \text{A--K--B} $ - Final products: $ \text{AB + K} $ **Multiple Choice Options:** A) Lowering the enthalpy of the reaction B) Lowering the activation energy of the reaction C) Changing the mechanism of the reaction D) Both A and B E) Both B and C *Reminder: Tap here or pull up for additional resources.*

$**Reaction Profile Explanation** This educational page describes a reaction profile comparing the pathway of a chemical reaction with and without a catalyst. **Text:** In the provided reaction profile, the black line represents the pathway of the reaction of A and B going to form AB. The red line represents the pathway when catalyst K is added. What is catalyst K doing in the reaction? **Diagram Explanation:** - The graph is a reaction profile chart with "Potential Energy" on the vertical axis and "Reaction Progress" on the horizontal axis. - The **black line** represents the uncatalyzed reaction pathway: - It starts at a certain energy level with reactants A and B. - The energy rises to a peak labeled as $ A \cdots B $, indicating the transition state. - The pathway then descends to a lower energy level at the products AB. - The **red line** shows the catalyzed reaction pathway with catalyst K: - The reaction begins with K + A + B at a similar energy level as the uncatalyzed pathway. - It goes through two smaller peaks labeled as $ K \cdots A + B $ and $ A \cdots K \cdots B $, indicating intermediate states. - The overall energy barrier is lower than the uncatalyzed path. - The pathway ends at AB + K, showing the regeneration of the catalyst. **Function of Catalyst K:** Catalyst K provides an alternative reaction pathway with a lower activation energy, increasing the reaction rate without being consumed in the overall process.$

Transcribed Image Text:**Reaction Profile Explanation** This educational page describes a reaction profile comparing the pathway of a chemical reaction with and without a catalyst. **Text:** In the provided reaction profile, the black line represents the pathway of the reaction of A and B going to form AB. The red line represents the pathway when catalyst K is added. What is catalyst K doing in the reaction? **Diagram Explanation:** - The graph is a reaction profile chart with "Potential Energy" on the vertical axis and "Reaction Progress" on the horizontal axis. - The **black line** represents the uncatalyzed reaction pathway: - It starts at a certain energy level with reactants A and B. - The energy rises to a peak labeled as $ A \cdots B $, indicating the transition state. - The pathway then descends to a lower energy level at the products AB. - The **red line** shows the catalyzed reaction pathway with catalyst K: - The reaction begins with K + A + B at a similar energy level as the uncatalyzed pathway. - It goes through two smaller peaks labeled as $ K \cdots A + B $ and $ A \cdots K \cdots B $, indicating intermediate states. - The overall energy barrier is lower than the uncatalyzed path. - The pathway ends at AB + K, showing the regeneration of the catalyst. **Function of Catalyst K:** Catalyst K provides an alternative reaction pathway with a lower activation energy, increasing the reaction rate without being consumed in the overall process.

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In the provided reaction profile, the black line represents the pathway of the reaction of A and B going to AB. The red line represents the pathway when catalyst K is added. What is catalyst K doing in the reaction? Potential Energy K + A + B AB K-A+B A-K-B KA + B AB+K