1. CHEMISTRY Matter and Change
Chapter 16: Reaction Rates

2. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Calculate average rates of chemical reactions from experimental data.
Relate rates of chemical reactions to collisions between reacting particles.
energy: the ability to do work or produce heat; it exists in two basic forms: potential energy and kinetic energy

3. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
reaction rate
collision theory
activated complex
activation energy
Collision theory is the key to understanding why some reactions are faster than others.

4. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Expressing Reaction Rates
The reaction rate of a chemical reaction is stated as the change in concentration of a reactant or product per unit of time.

5. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Expressing Reaction Rates (cont.)
Reaction rates are determined experimentally.

6. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Collision Theory
Collision theory states that atoms, ions, and molecules must collide in order to react.

7. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Collision Theory (cont.)
An activated complex is a temporary, unstable arrangement of atoms in which old bonds are breaking and new bonds are forming.

8. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Collision Theory (cont.)
The minimum amount of energy that reacting particles must have to form the activated complex and lead to a reaction is called the activation energy.
High activation energy means that few collisions have the required energy and the reaction rate is slow.

9. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Collision Theory (cont.)

10. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Collision Theory (cont.)

11. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Collision Theory (cont.)

12. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Spontaneity and Reaction Rate
Are more spontaneous reactions faster than less spontaneous reactions?
ΔG indicates only the natural tendency for a reaction to proceed—it does not affect the rate of a chemical reaction.

13. SECTION16.1
Section Check
Which of the following is NOT a requirement for a reaction to occur, according to the collision theory?
A. Reacting substances must collide.
B. Reacting substances must be in an exothermic reaction.
C. Reacting substances must collide in the correct orientation.
D. Reacting substances must collide with sufficient energy to form an activated complex.

14. SECTION16.1
Section Check
A temporary, unstable arrangement of atoms in which old bonds are breaking and new bonds are forming is called ____.
A. reaction complex
B. reaction substrate
C. activated complex
D. activated molecule

15. A Model for Reaction Rates
SECTION16.1
A Model for Reaction Rates
Study Guide
Key Concepts
The rate of a chemical reaction is expressed as the rate at which a reactant is consumed or the rate at which a product is formed.
Reaction rates are generally calculated and expressed in moles per liter per second (mol/(L ● s)).
In order to react, the particles in a chemical reaction must collide.
The rate of a chemical reaction is unrelated to the spontaneity of the reaction.

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