* During energy transformations in living systems, order and organization must be compensated by releasing energy which will increase entropy of the surrounding. 
* Organisms are open systems that exchange materials and energy with the environment. They are never at equilibrium with the surrounding. 
* Energy is spent to create and maintain order in the cells, and surplus energy and other simpler by-products are released to create disorder such that there is an increase in entropy of the surrounding. 
* In a reversible process, entropy remains constant where as in an irreversible process (more common to real-world scenarios), entropy tends to increase. 
* During phase changes (from solid to liquid, or to gas), entropy increases because the number of possible arrangements of particles increases. 
* If ∆G<0, the chemical reaction is spontaneous and favourable in that direction. 
* If ∆G=0, the reactants and products of chemical reaction are at equilibrium. 
* If ∆G>0, the chemical reaction is non-spontaneous and unfavorable in that direction. 
* ∆G is not an indicator for velocity or rate of chemical reaction at which equilibrium is reached. It depends on amount of enzyme and energy activation.