CHEM1100 Lecture Notes - Lecture 17: Standard Molar Entropy, Spontaneous Process, Thermodynamics
Lecture 17 - Spontaneity and entropy !
Notes about spontaneous reactions
•Can occur without outside intervention (no input of energy) #
•Thermodynamics tells us about the direction of a process – not its speed. #
•Thermodynamically a diamond should change spontaneously to graphite, however it is a very
slow process #
•There is nothing in the definition of ‘spontaneous’ that describes how FAST the process is. !
•Kinetics tells us how fast a reaction is. "
•Thermodynamics tells us if it will proceed at all. "
Entropy
•The measure of overall distribution of positions and energies in a system (the probability of a
system).!
•It is the driving force for spontaneity.!
•entropy is based off the probability of distribution. !
•Temperature effects entropy: the higher temperature, the greater the entropy due to molecule
vibration and spreading out !
Second law of thermodynamics: entropy
In any spontaneous process there is always an increase in the total entropy of the universe. !
∆S > 0 : entropy increases: process is spontaneous !
∆S < 0 : entropy deceases: process is spontaneous in the opposite direction !
∆S = 0 : equilibrium !
!
Measuring entropy
!
Standard molar entropy
The entropy of 1 mole of substance#
q = C ΔT
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