How does cooling a reaction affect the rate of the reaction? (Hint: Use collision theory to answer this question) a. The rate of reaction is decreased since the reactants have less potential energy. b. The rate of reaction is increased as less collisions occur due to a decrease in the speed of the reactants. c. The rate of the reaction is increased as more collisions occur due to an increase in successful collisions. d. The rate of the reaction is decreased as the number of successful collisions decrease due to the reactants having less kinetic energy. e. The rate of the reaction is decreased as the number collisions with the correct activation energy decreases.
How does cooling a reaction affect the rate of the reaction? (Hint: Use collision theory to answer this question) a. The rate of reaction is decreased since the reactants have less potential energy. b. The rate of reaction is increased as less collisions occur due to a decrease in the speed of the reactants. c. The rate of the reaction is increased as more collisions occur due to an increase in successful collisions. d. The rate of the reaction is decreased as the number of successful collisions decrease due to the reactants having less kinetic energy. e. The rate of the reaction is decreased as the number collisions with the correct activation energy decreases.
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter16: Reaction Rates
Section: Chapter Questions
Problem 87A
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Transcribed Image Text:How does cooling a reaction affect the rate of the reaction? (Hint: Use collision theory to answer this
question)
a. The rate of reaction is decreased since the reactants have less potential energy.
b. The rate of reaction is increased as less collisions occur due to a decrease in the speed of the
reactants.
c. The rate of the reaction is increased as more collisions occur due to an increase in successful
collisions.
d.
The rate of the reaction is decreased as the number of successful collisions decrease due to the
reactants having less kinetic energy.
e. The rate of the reaction is decreased as the number collisions with the correct activation energy
decreases.
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