Gibbs Free Energy
G = ΔH - TΔS; if G > O then non-spontaneous
Reaction that’s Spontaneous at ALL Temperatures at Standard Pressure and Concentration
Exothermic reaction with an increase in entropy
Reaction that’s Spontaneous at HIGH Temperatures at Standard Pressure and Concentration
Endothermic reaction with an increase in entropy
Reaction that’s Spontaneous at LOW Temperatures at Standard Pressure and Concentration
Exothermic reaction with a decrease in entropy
Reaction that’s Spontaneous at NO Temperatures at Standard Pressure and Concentration
Endothermic reaction with a decrease in entropy
Hess’s Law
The enthalpy change of a reaction is the same regardless of the path
Phase change of enthalpy of fusion (ΔHfus)
Solid → Liquid
Phase change of enthalpy of vaporization (ΔHvap)
Liquid → Gas
Phase change of enthalpy of sublimation (ΔHsub)
Solid →Gas
Zeroth Law of Thermodynamics
If two systems are each in thermal equilibrium with a third system, they are in thermal equilibrium with each other
The First Law of Thermodynamics
Energy cannot be created or destroyed, only transformed
The Second Law of Thermodynamics
Every energy transfer or transformation increases the entropy of the universe
The Third Law of Thermodynamics
As the temperature approaches absolute zero, the entropy of a perfect crystal approaches zero
