1. Zero law
1.1. Thermal equilibrium
1.1.1. Heat transfers to cold
2. First Law
2.1. Conservation of Energy
2.1.1. delta E=Q-W
2.1.1.1. Q_W=delta U+ delta Ec+ delta Ep
3. Second law
3.1. Entropy
3.1.1. delta S total is greater than 0
3.1.1.1. Deal with spontaneous or not of a process
3.1.1.1.1. Spontaneous doesnt require work or energy to happen
3.1.1.1.2. Non-spotaneous require work or energy to happen
3.1.1.2. The direction of spontaneous change is determined by the distribution of energy
3.2. Any spontaneous process must be accompanied by an increase in the total delta S total of system and surrounding
3.2.1. Condition for equilibrium
3.2.1.1. dS_tot=dSy_sstem+dS_surrounding=0
4. Phase change
4.1. When the state matter changes due to deltaH
4.1.1. DeltaH=rxn heta,latent heat,sensible heat
4.2. Phase is in equilibrium when deltaStransition=deltaHtransition/Ttransition=0
4.3. Endothermic
4.3.1. deltaHtransition>0
4.3.2. deltaStransition>0
5. Max Welll reltations
5.1. relations of non mesurable variables to mesurable variables
6. Fugacity
6.1. porpotional to gibbs freee energy
6.2. Tendency to escape the phase
6.3. Concentration depends on phase
7. Enthalpy
7.1. Of reaction
7.1.1. deltaH=deltaH_rxn=deltaH_products-deltaH_reactants
7.1.2. deltaH>0, endothermic
7.1.3. deltaH<0, exothermic
7.2. Standard enthalpies of formation
7.2.1. heat changes the result when 1 mole of a compound is formed from its consituent elemnts in standard state
7.2.2. standard state is the most stable state at 1 atm
7.2.3. delta H _f for elements in stable state=0
8. Steady state
8.1. no change over time dx/dt=0
8.2. It's not static it just doesn't change with t
9. Equilibrium
9.1. Lack of change delta S=0
9.1.1. Driving forces are in exact balance
9.2. Lack of change
10. Equilbrium state is the one with maximum entropy
10.1. dStotal=dSsystem+ dSsurroundings
10.2. dStotal=dqsystem/Tsystem
10.3. dq-Tds=0
10.3.1. Clausius Inequality
10.4. If a process is possible deltaS>0
10.5. Thermal eq.=Tsystem=Tsurroundings; delta T=0
10.5.1. thermal, mechanical, chemical delta=0 simultaneously
10.6. Mechanical eq.=Psystem=Psurroundings; delta P=0
10.7. Chemical eq.stet where species have no tnedency to change can happen with one or more phase; delta G=0
10.8. Criteria 1° and 2° law Thermo. dG=dH-Tds Gibbs free energy
11. Gibbs free energy
11.1. Gi=Hi-Tsi
11.2. Thermo. property to determine spontaniety of process
11.3. deltaG<o spontaneous; deltaG>0 non spontaneous; deltaG=0 condition for chemical equilibrium
12. Phase equilibrium
12.1. Claperon ecuation
12.1.1. Sloid to liquid=P2=P1+deltaH/deltaV ln T2/T1
12.1.2. Liquid to vapor Pe=P1*e^-(deltaH/R(1/T2-1/T1))=Clausius Clapeyron
13. Direction of an spontaneous change
13.1. Not related to amount of energy
13.1.1. proved by the fisrt law