1. (Collision theory, Kinetic theory) explain how collision between reactant molecules may or may not result in a successful chemical reaction. 2. Chemical reaction rate increases/ decreases with an increase/ decrease in (temperature, energy). 3. (Active energy, activation energy) is the minimum amount of energy needed for a reaction to occur. 4. Chemical reaction can only happen when the (reactant, product) particles collide with each other. 5. (Energy graph, energy diagram) are used to analyze the changes in energy that occur during a chemical reaction. 6. (Regrouping, separating ) of atoms causes chemical reaction. 7. Chemical reaction can't take place when there is an (effective , ineffective ) collision of atoms/molecules. 8. (Catalyst , solution ) can lower 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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Read the statement carefully. Choose & encircle the correct answer in the parenthesis

1. (Collision theory, Kinetic theory) explain how collision between reactant molecules may or may not result in a
successful chemical reaction.
2. Chemical reaction rate increases/ decreases with an increase/ decrease in (temperature, energy).
3. (Active energy, activation energy) is the minimum amount of energy needed for a reaction to occur.
4. Chemical reaction can only happen when the (reactant, product) particles collide with each other.
5. (Energy graph, energy diagram) are used to analyze the changes in energy that occur during a chemical
reaction.
6. (Regrouping, separating ) of atoms causes chemical reaction.
7. Chemical reaction can't take place when there is an (effective , ineffective ) collision of atoms/molecules.
8. (Catalyst , solution ) can lower the activation energy.
Transcribed Image Text:1. (Collision theory, Kinetic theory) explain how collision between reactant molecules may or may not result in a successful chemical reaction. 2. Chemical reaction rate increases/ decreases with an increase/ decrease in (temperature, energy). 3. (Active energy, activation energy) is the minimum amount of energy needed for a reaction to occur. 4. Chemical reaction can only happen when the (reactant, product) particles collide with each other. 5. (Energy graph, energy diagram) are used to analyze the changes in energy that occur during a chemical reaction. 6. (Regrouping, separating ) of atoms causes chemical reaction. 7. Chemical reaction can't take place when there is an (effective , ineffective ) collision of atoms/molecules. 8. (Catalyst , solution ) can lower the activation energy.
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