1. Spontaneity

2. Spontaneous reactions
Spontaneous reactions occurs with NO INPUT OF ENERGY
Spontaneous reactions allow for the transfer of electrons from an oxidizing agent to a reducing agent

3. Testing spontaneity How could you test spontaneity?
Place 2 substances in contact and see if they react!

4. Spontaneity rule
If the oxidizing agent is HIGHER (on the spontaneity chart) than the reducing agent, the reaction will be spontaneous

5. USES Spontaneous reactions produce energy!
What could we use this for??

6. Label the Oxidizing agents from strongest to weakest according to the chart* C+ D+

7. Example 2
In a children’s chemistry set, a common reaction involves placing Iron shavings into a solution of Copper(II)Sulfate. Predict the spontaneity of this reaction.

8. Sacrificial Anodes AKA galvanic cathodic protection
Used to protect buried or submerged metal structures from corrosion

9. Sacrificial anodes are made from a more “active” metal and will oxidize in place of the metal pipe
Where would the sacrificial anode need to be (on the chart) in order to oxidize before the metal pipe???

10. Example 3
Determine 3 sacrificial anodes that the oil industry could use to reduce the oxidation of iron in steel pipes. List 1 pro and 1 con for each metal used