1. Chapter 20: Chemical Reactions and Energy
Thermodynamics
What is Energy?
2 Main Types: Potential and Kinetic
Potential – energy of composition or position
Kinetic – energy of motion

2. Chemical Systems contain both Potential and Kinetic Energy
Energy can change form or flow but its always conserved.
Takes energy to break bonds and energy is released when bonds are formed
Law of Conservation of Mass and Energy – energy is neither created or destroyed in a chemical reaction.
Also known as the 1st Law of Thermodynamics
Heat Energy – symbol is q
– always flows from hot to cold
Units of Energy are Joules (J) or kilojoules (kJ)

3. Energy Diagrams are used to illustrate energy changes in chemical reactions.
When the energy stored in the products is less than the reactants, energy has been given off.
Exothermic reaction – energy given off to the environment. Products are at a lower energy level than the reactants.

4. Endothermic Reactions
When the products are at a higher energy level (system absorbed energy) than the reactants.

5. Formula: ∆H reaction = ∆ H products - ∆ H reactants
The difference in energy between products and reactants in a chemical reaction is given the symbol ∆ H (delta H)
∆ symbol means difference or change. Also known as Enthalpy
∆ H = enthalpy = heat energy lost or gained
Formula: ∆H reaction = ∆ H products - ∆ H reactants
Formula: ∆Hrxn = ∆Hprod - ∆Hreact
In Exothermic reactions the energy stored in products is less than in reactants
∆ H is negative

6. Endothermic reactions energy stored in products is greater than that of the reactants.
∆ H is positive
Input of energy is called Activation Energy (Ea)
Required in both Endothermic and Exo Reactions

7. B = Activation Energy difference in energy between the reactants and the maximum energy
A= reactants
B= Activation energy
C= Activated complex
D= ΔH
E= products

8. How do catalysts effect the rate of a reaction?
Two curves are shown in the following energy diagram. Which represents the catalyzed reaction?
Red curve
Catalysts lower the activation energy

9. Reaction without a catalyst
Reaction with a catalyst

10. A Catalytic Converter
Exhaust gases from an automobile pass through a two-stage catalytic converter. In one stage, carbon monoxide and unburned hydrocarbons are converted to carbon dioxide and water. In the second stage, NO is converted to nitrogen gas and oxygen gas.

11. Forces that Drive Chemical Reactions
Why do some reactions occur spontaneously? (fast without a catalyst)
3 Factors are involved: Order, Disorder and Entropy
Entropy – describes disorder. Not conserved. Used to describe and measure the degree of disorder.
Ice melting – classic example of entropy increasing

12. The mixture on the right has more disorder and a higher entropy than the mixture on the left

13. Systems tend to go from a state of high energy (∆H) to a state of low energy (more stable state). Exothermic reactions more common.
Systems tend to become more disordered – greater entropy.
Spontaneous reactions tend to occur if energy decreases and if disorder increases (exothermic).
The Direction of a Chemical reaction - In room temp. most exothermic reactions tend to be spontaneously in the forward direction.