1. Entropy

2. 1 st Law of Thermodynamics Energy is neither created nor destroyed –The energy of the universe is constant –Energy just changes from one form to another This law lets us know the energy of the system, but does not give us any information about the direction of the energy flow

3. Spontaneity Spontaneous process – a process that occurs without intervention –Spontaneous processes can be fast or slow Spontaneity tells us the direction of the energy flow –It tells us NOTHING about the speed of the reaction

4. For example… A ball spontaneously rolls down a hill –It does not spontaneously roll up If iron is exposed to air, it spontaneously rusts –The rust does not spontaneously turn back into air & iron

5. Entropy Entropy (s) – the measure of molecular randomness or disorder –Think of entropy as the amount of chaos The driving force for a spontaneous process is an increase in entropy

6. Entropy The natural progression of things is from order to disorder Or from lower entropy to higher entropy –Think of a deck of cards…when you drop one it goes from order to disorder –Think of your room… it goes from order to disorder Think if entropy as a probability…not a certainty –Nature spontaneously proceeds toward that states that have the highest probability of existing

7. Entropy Predict which has the highest entropy 1.CO 2 (s) or CO 2 (g) CO 2 (g) 2.1 mol of N 2 at 1 atm or 1 mol of N 2 at 0.001 atm 1 mol of N 2 at 0.001 atm

8. Entropy Predict the sign of the entropy change for the following… 1.Sugar is added to water to form a solution + 2.Iodine vapor condenses on a cold surface to produce a liquid -

9. 2 nd Law of Thermodynamics 2 nd Law of Thermodynamics – In any spontaneous process there is always an increase in entropy of the universe Energy is conserved…entropy is NOT conserved! The entropy of the universe is always increasing –  S univ = + = spontaneous –  S univ = - = not spontaneous (would be spontaneous in the opposite direction) –  S univ = 0 = no tendency to occur (system is at equilibrium)  S univ =  S sys +  S surr

10. Temperature & Spontaneity  S surr = _  H T T must be in Kelvin  H is usually given in KJ/mol  S will be in KJ/K, but is usually changed to J/K

11. Example Sb 2 S 3 (s) + 3Fe (s)  2Sb (s) + 3FeS (s)  H = -125 kJ Calculate  S surr for this reaction at 25  C and 1 atm  S = - (  H/T)  S = - (-125KJ/298K)  S = 0.419 KJ/K  S = 419 J/K

12. Example Sb 4 O 6 (s) + 6C (s)  4Sb (s) + 6CO (g)  H = 778 kJ Calculate  S surr for this reaction at 25  C and 1 atm  S = - (  H/T)  S = - (778KJ/298K)  S = -2.61 KJ/K  S = -2610 J/K

13. 3 rd Law of Thermodynamics The entropy of a perfect crystal at 0K is zero

14. Free Energy Free energy (G) – a thermodynamic function equal to the enthalpy minus the product of the entropy and the Kelvin temperature  G =  H – T  S A process is only spontaneous in the direction where  G is negative

15. Example At what temperatures is the following process spontaneous at 1 atm? –Br 2 (l)  Br 2 (g) –  H = 31.0 KJ/mol  31000 J/mol –  S = 93.0 J/ K mol  G =  H – T  S 0 = 31000 – T(93.0) T = 333K Above 333K the reaction is spontaneous

16. Dependence of H & S on Spontaneity HH SS Result -+ ++ -- +-  G =  H-T  S Spontaneous at all temperatures Spontaneous at high temperatures Spontaneous at low temperatures Not spontaneous at any temperature