The theoretical effect of an increase in the initial concentration of a reactant can be explained in terms of collision theory because it affects the collision geometry involved in the reaction the total number of collisions that occur I. II. III. IV. the fraction of collisions that are effective the required activation energy for a reaction Select one: O a. O b. O c. d. Il only both I and IV both II and III both III and IV

The theoretical effect of an increase in the initial concentration of a reactant can be explained in terms of collision theory because it affects the collision geometry involved in the reaction the total number of collisions that occur I. II. III. IV. the fraction of collisions that are effective the required activation energy for a reaction Select one: O a. O b. O c. d. Il only both I and IV both II and III both III and IV

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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3. When 6 g of granulated Zn is added to a solution of 2 mol/L HCI in a beaker at room temperature, hydrogen gas is generated. For each of the following changes (constant volume of the acid), state whether the rate of hydrogen gas evolution will be increased, decreased, or unchanged. Explain using collision theory. a. 6 g of powdered Zn is used. b. 4 g of granulated Zn is used. c. Temperature is raised to 40°C.
The frequency factor in the Arrhenius equation can best be described as O a. a factor which corrects for the conversion between J and kJ. O b.a numerical description of the amount of energy needed by colliding reactant molecules in order to form products. Oc the probability that a collision between molecules will have the corect relative orientation for reaction to occur. d.a numerical description of the amount of energy released by colliding reactant molecules when they form products. e. a numerical description of how often molecules collide with the proper orientation to react ar a specific concentration.
Which of the following will decrease the activation energy, Ea, of a reaction? O Increasing the reactant concentrations Removing the products as they form O Increasing the temperature O Adding a catalyst O Decreasing the pressure A Moving to another question will save this response. M esc 20 F3 F1 F2 F4 F5 @ #3 24 4 Q W R. A
16. How can the effect of temperature on the reaction rate be explained by collision theory?
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Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
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Hw.38.
16. A reaction mechanism proposes three step reactions for the overall reaction and the energy diagram shows three activated states. From the proposed mechanism and energy diagram how many reaction intermediates are expected to form?A. 3 B. none C. 1 D. 2 E. 4
A zero extent of reaction indicates: a. reversible reaction b. no reaction c.equilibrium system d. steady-state system
12. Three concentration-time graphs for chemical reactions are shown below: Graph 1 Graph 2 Graph 3 [X] [X] [X] Time Time Time Which of the three graphs correctly shows a reaction in which the concentration of the reactant X would affect the rate of the reaction? a. Graph 1 only b. Graph 2 only c. Graphs 1 and 3 d. Graphs 1 and 2