Answered: I need help with this diagram because I…

Biology 2e

2nd Edition

ISBN:9781947172517

Author:Matthew Douglas, Jung Choi, Mary Ann Clark

Publisher:Matthew Douglas, Jung Choi, Mary Ann Clark

Chapter6: Metabolism

Section: Chapter Questions

Problem 1VCQ: Figure 6.8 Look at each of the processes shown, and decide if it is endergonic or exergonic. In each...

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I need help with this diagram because I wrote the wrong Mark for Gp, Gr And I have to represent *triangle* G, Ea without the enzyme and Ea with the enzyme. And when I put that down it looked wrong so I need help with labeling this diagram so that I can practice this more on the future

$### Free Energy Diagram of a Chemical Reaction This diagram illustrates the changes in free energy that occur during a chemical reaction. The x-axis represents the progress of the reaction, while the y-axis shows the free energy. Here is a detailed explanation of the diagram: 1. **Reactants and Products**: - On the left side of the diagram, the reactants $A$ and $B$ have a certain amount of free energy. - As the reaction progresses from left to right, the reactants convert to products $C$ and $D$ on the right side of the diagram. 2. **Activation Energy (Without and With Catalyst)**: - The energy profile shows two curves: one with a higher peak (solid line) and another with a lower peak (dashed line). - **Without Catalyst**: - The peak of the solid line represents the activation energy (denoted by $a$) required for the reaction to proceed in the absence of a catalyst. - **With Catalyst**: - The peak of the dashed line represents the lower activation energy (denoted by $b$) when a catalyst is present. 3. **Energy Differences**: - $c$: The free energy difference between the reactants ($A + B$) and the top of the energy barrier (activation energy) without a catalyst. - $d$: The free energy difference between the products ($C + D$) and the activation energy with a catalyst. - $e$: The overall change in free energy from reactants to products, indicating whether the reaction is exergonic or endergonic. 4. **Energy States**: - Initially, the reactants are at a higher energy state. - The energy increases to reach the transition state (highest point on the curve). - After crossing the transition state, the energy decreases, forming the products which are at a lower energy state compared to the reactants. This diagram effectively demonstrates how a catalyst lowers the activation energy barrier, facilitating the reaction to proceed more easily. It is a crucial concept in understanding how catalysts function to accelerate chemical reactions without being consumed in the process.$

Transcribed Image Text:### Free Energy Diagram of a Chemical Reaction This diagram illustrates the changes in free energy that occur during a chemical reaction. The x-axis represents the progress of the reaction, while the y-axis shows the free energy. Here is a detailed explanation of the diagram: 1. **Reactants and Products**: - On the left side of the diagram, the reactants $A$ and $B$ have a certain amount of free energy. - As the reaction progresses from left to right, the reactants convert to products $C$ and $D$ on the right side of the diagram. 2. **Activation Energy (Without and With Catalyst)**: - The energy profile shows two curves: one with a higher peak (solid line) and another with a lower peak (dashed line). - **Without Catalyst**: - The peak of the solid line represents the activation energy (denoted by $a$) required for the reaction to proceed in the absence of a catalyst. - **With Catalyst**: - The peak of the dashed line represents the lower activation energy (denoted by $b$) when a catalyst is present. 3. **Energy Differences**: - $c$: The free energy difference between the reactants ($A + B$) and the top of the energy barrier (activation energy) without a catalyst. - $d$: The free energy difference between the products ($C + D$) and the activation energy with a catalyst. - $e$: The overall change in free energy from reactants to products, indicating whether the reaction is exergonic or endergonic. 4. **Energy States**: - Initially, the reactants are at a higher energy state. - The energy increases to reach the transition state (highest point on the curve). - After crossing the transition state, the energy decreases, forming the products which are at a lower energy state compared to the reactants. This diagram effectively demonstrates how a catalyst lowers the activation energy barrier, facilitating the reaction to proceed more easily. It is a crucial concept in understanding how catalysts function to accelerate chemical reactions without being consumed in the process.

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