9. An increase in temperature increases the reaction rate. What is the best reason to explain this effect? A. a greater fraction of the collisions have the correct orientation of molecules B. the activation energy of the reaction will increase C. the activation energy of the reaction will decrease D. more collisions will have enough energy to exceed the activation energy

9. An increase in temperature increases the reaction rate. What is the best reason to explain this effect? A. a greater fraction of the collisions have the correct orientation of molecules B. the activation energy of the reaction will increase C. the activation energy of the reaction will decrease D. more collisions will have enough energy to exceed the activation 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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Similar questions

Describe two ways to make a chemical reaction proceed faster, and explain why the rate increases according to collision theory.
Addition of a catalyst to a reaction lowers the activation energy of at least one step in the reaction
Which statements regarding the collision model are true? A. Molecules must collide with one another for a chemical reaction to occur. B. Molecules must be aligned with specific orientation for collisions between them to result in chemical reactions. C. All collisions between molecules result in chemical reactions. D. Collisions between molecules that occur with more than a minimum amount of energy always result in chemical reactions. E. Molecules must collide both with a minimum amount of energy and with the appropriate orientation relative to each other to result in chemical reactions.
1. a. Explain in your own words, what is meant by the term "activation energy." b. How can the idea of activation energy be used to explain the temperature dependance of rate? c. How can activation energy be used to explain why a catalyst increases the rate of a chemical reaction
What is the difference between exergonic and exothermic? What is the difference between intermediate and transition state? What is the relation between activation energy and the rate of a reaction?
Which one of the following factors does not affect the specific rate constant of a chemical reaction? A. Arrhenius probability factor B. Amounts of reactants C. Temperature D. The presence of a catalyst E. Activation barrier
What does a catalyst do to speed the reaction rate? It increases the concentration of the reactants. It lowers the activation energy. O It increases the kinetic energy of the reactants. It increases the temperature of the reaction. O It increases the number of collisions between the reactants.
40. The reaction that produces ammonia is represented by a balanced equation, shown below. A catalyst can be used to increase the rate of the reaction. N2(g) + 3H2(g) → 2NH3(g) + energy A potential energy diagram for the reaction is shown below. C A Reaction Coordinate What occurs when a catalyst is added to a chemical reaction? A. an alternate reaction pathway lowers activation energy, changing the magnitude of both B and C B. new reactants are added which increases their potential energy, changing the magnitude of both A and D C. different products are produced with a lower potential energy, changing the magnitude of both A and B D. the temperature is increased so there are more effective collisions, which changes the magnitude of A and C
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