Explain, using Collison theory, one factor effecting the rate of a reaction. Draw a potential energy diagram given the following information. the reaction proceeds in three steps the activation energy of step 2 is double that of step 1. • the activation energy of step 3 is double that of step 2 the reaction is endothermic Label all axes, the rate limiting step, the location of any intermediates and transition states, the overall enthalpy of reaction, the reactants and products. Using a dotted line, show the effects of a catalyst on the reaction and provide a brief explanation.

Explain, using Collison theory, one factor effecting the rate of a reaction. Draw a potential energy diagram given the following information. the reaction proceeds in three steps the activation energy of step 2 is double that of step 1. • the activation energy of step 3 is double that of step 2 the reaction is endothermic Label all axes, the rate limiting step, the location of any intermediates and transition states, the overall enthalpy of reaction, the reactants and products. Using a dotted line, show the effects of a catalyst on the reaction and provide a brief explanation.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 106CP: Most reactions occur by a series of steps. The energy profile for a certain reaction that proceeds...

See similar textbooks

Similar questions

Account for the relationship between the rate of a reaction and its activation energy.
Consider the following hypothetical reaction: X+YProductsH=75kJ Draw a reaction-energy diagram for the reaction if the activation energy is 32 kJ.
The reaction of H2 molecules with F atoms H2(g) + F(g) HF(g) + H(g) has an activation energy of 8 kJ/mol and an enthalpy change of 133 kJ/mol. Draw a diagram similar to Figure 14.11 for this process. Indicate the activation energy and enthalpy change on this diagram.
How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate.
Use the PhET Reactions Single collision" tab of the simulation applet, enable the Energy view by clicking the + icon. Select the first A+BCAB+C reaction] (A is yellow, B is purple, and C is navy blue). Using the straight shot default option, try launching the A atom with varying amounts of energy. What changes when the Total Energy line at launch is below the transition state of the Potential Energy line? Why? What happens when it is above the transition state? Why?
Most reactions occur by a series of steps. The energy profile for a certain reaction that proceeds by a two-step mechanism is On the energy profile, indicate a. the positions of reactants and products. b. the activation energy for the overall reaction. c. E for the reaction. d. Which point on the plot represents the energy of the intermediate in the two-step reaction? e. Which step in the mechanism for this reaction is rate determining, the first or the second step? Explain.
Consider a reaction in which E a=129 kJ and H=29 kJ. In the presence of a catalyst, the activation energy is 48% of the uncatalyzed reaction. Follow the directions in Question 71 in drawing an energy diagram.
For the following reaction profile, indicate a. the positions of reactants and products. b. the activation energy. c. E for the reaction.