Chapter 19 - Thermodynamics Flashcards
Spontaneous processes
Those that can proceed without outside intervention.
Non spontaneous in reverse direction
Temperature matters!
First law of thermodynamics
Energy cannot be created or destroyed
Total energy of universe is constant
Can be converted
Reversible process
System and surroundings can be put back to original state by exactly reversing the process
Irreversible process
Cannot be undone
Spontaneous processes are irreversible
Entropy
Measure of randomness
Related to motion in molecules
Change in entropy equals entropy final minus entropy initial
q/t
Isothermal process
A process occurring at constant temperature
For entropy the change is equal to heat that would be transferred if reversible divided by temperature
Second law of thermodynamics
Entropy of the universe increases for spontaneous processes and does not change for reversible processes
Entropy of universe always increasing
Average kinetic energy
Temperature
Motion of molecules
Translational: movement of entire molecule from one place to another
Vibrational
Rotational: rotation of molecule about axis or sigma bonds
Microstate
Snapshot of molecule notion in a thermodynamic system
Entropy equation with microstates
S= k lnW
K is 1.38e-23
W is microstates
Number of microstates increase when
Entropy increases
Temperature increases
Volume increases
Molecules increase
Entropy in solutions
When solid is dissolves in a solvent, entropy increases
Third law of thermodynamics
The entropy of pure crystalline substance at absolute zero is 0
Standard entropies
Molar entropy values of substances in their standard state
Tend to increase with increasing molar mass