Consider the following potential energy diagram: Reaction coordinate Which path represents a catalyzed reaction? How many steps would be proposed in the mechanism for the catalyzed reaction, and which step would be rate-determining? Since there are activation energies shown for the catalyzed reaction there are steps in the mechanism. The slowest step would be the step in the mechanism as that step has the activation energy of the v in the mechanism. Potential energy

Consider the following potential energy diagram: Reaction coordinate Which path represents a catalyzed reaction? How many steps would be proposed in the mechanism for the catalyzed reaction, and which step would be rate-determining? Since there are activation energies shown for the catalyzed reaction there are steps in the mechanism. The slowest step would be the step in the mechanism as that step has the activation energy of the v in the mechanism. Potential energy

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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Study the following reaction energy diagram: energy reactants Then answer the following questions about the chemical reaction. Does this reaction release or absorb energy? How many transition states occur during this reaction? Could this be an elementary reaction? If you said this reaction could not be elementary, then how many steps are in its mechanism? If you said this reaction could not be elementary, then enter the number of the step in its mechanism which is rate- determining. For example, if the first step is the rate- determining step, enter "1" here. 0 products release absorb neither yes no
How does subdividing (grinding up) the reactants affect the rate of a chemical reaction? O It decreases the rate by giving the reactants the wrong orientation for reacting. O It increases the rate by lowering the energy of activation (E,). O It increases the rate by giving more molecules enough energy to react. O It decreases the rate by raising the energy of activation (E). O It increases the rate by increasing the surface area or effective concentration of the reactants.
A burner in a gas stove breaks propane and oxygen up to form carbon dioxide and water, thereby heating a home. Which part is the source of the activation energy required, and is this reaction endothermic or exothermic? The flame from the burner provides the energy to perform the reaction. The reaction is endothermic. The burning propane gas provides the energy to perform the reaction. The reaction is exothermic. The burning propane gas provides the energy to perform the reaction. The reaction is endothermic. The flame from the burner provides the energy to perform the reaction. The reaction is exothermic.
Which one of the following statements is False? The rate constant depends on the activation energy of a reaction. A catalyst lowers the activation energy of a reaction. Rate constants are not temperature dependent.
po Energy and Matter Transition States At the peak of the Reaction Pathways graph, there is a brief interval between the time that the reactant bonds are broken and product bonds are formed. This transitional structure is called an activated complex, and it exists for only a brief period of time. Just because the activated complex forms does not necessarily mean products will form. It may return to the original reactants, Increasing the temperature of the reaction causes more particles to have sufficient energy to form the activated complex on collision. That is why reaction rate increases as temperature increases. Increasing temperature increases the opportunities for products to form. APPLY How does concentration affect the formation of the activated complex? Haughton Miflin Harcourt Publishing Company
Consider a hypothetical chemical reaction A + B → C, where A and B are reactants and C is the product. The reaction is known to have a high activation energy barrier. However, upon adding a catalyst, the reaction proceeds at a significantly faster rate. Explain the role of the catalyst in reducing the activation energy barrier and increasing the reaction rate.
Question: Consider a hypothetical chemical reaction between compound A and compound B. The reaction is exothermic and yields compound C and compound D as products. The reaction mechanism involves multiple elementary steps. Based on this information, answer the following questions: Define the terms "exothermic reaction" and "endothermic reaction" and provide an example of each. Explain the concept of a reaction mechanism and why it is important in understanding chemical reactions. Outline the steps involved in determining the rate-determining step in a reaction mechanism. Describe how a catalyst affects the rate of a chemical reaction and provide an example of a catalyst commonly used in industrial processes. Given that the reaction between compound A and compound B is exothermic, suggest one possible reason why the reaction might still have a high activation energy.
For a reaction with activation energy of 44 kJ and heat of reaction of -31 kJ and product energy of 90. kJ, what is the reactant energy level? Question 5 options: 134 121 46 103 59 13
Consider the two-step mechanism for the destruction of ozone. step 1: 0,(g) + HO(g) HO, (g) + 0,(g) > step 2: HO, (g) + O(g) → HO(g) + 0,(g) Identify the type of catalyst. Identify the catalyst in the two-step mechanism. homogeneous catalyst O heterogeneous catalyst O, НО HO2
Increasing the temperature of a reaction increases the speed at which the reaction occurs. Identify the statements that explain the correlation between the increase in temperature and the increase in reaction rate. More atom-atom stretching and bending within the molecules occurs at higher temperatures, which creates more reactive molecular configurations. Added heat decreases the activation energy of a reaction and has a similar effect as adding a catalyst. ✔ Molecules at higher temperatures have greater kinetic energy, which results in more frequent and higher energy collisions. An increased temperature improves the reaction pathway by decreasing the energy difference between reactants and products.
Which of the following is true? Decreasing the activation energy decreases the reaction rate. Decreasing the activation energy increases the reaction rate. The activation energy of an exothermic reaction is negative. There is no relationship between activation energy and reaction rate.
Which is true? A slow reaction has low activation energy. A fast reaction has large activation energy. The size of the activation energy tells us about the reaction rate. The size of the activation energy tells us about the reaction mechanism.