Thermodynamics Flashcards
Spontaneous change
one that occurs without a continuous input of energy from outside the system (though activation energy may be required to initiate it)
If a change is spontaneous in one direction
it will be non-spontaneous in the reverse direction
how may non-spontaneous reactions and processes be driven?
with continual input of energy
is enthalpy change a predictor of spontaneity?
many exothermic processes are spontaneous (eg combustion reactions)
examples of spontaneous endothermic transformations
- melting of ice (at higher temps)
- dissolution (of some solids at some concentrations and temps)
all show an increase in the freedom of motion of particles in the system
relationship between freedom of motion and spontaneity
an increase in freedom of motion (dispersal of energy) favours spontaneity
entropy, S
measure of energy dispersal, or freedom of motion, in a system
positive value of ΔS indicates
negative value of ΔS indicates
increased dispersal of energy
decreased dispersal of energy
is entropy a state function?
yes
ΔS = S(final) - S(initial)
units of entropy
J/K
S’
standard molar entropy: entropy of 1 mole of the pure substance in its standard state
entropy trends
- effect of physical state
- effect of particle numbers
- effect of molecular complexity
- effect of temperature
effect of physical state
S of solids < S of liquids «_space;S of gas
solids - less energy dispersed, lower entropy
effect of particle numbers
more molecules have higher entropy than fewer molecules
effect of molecular complexity
entropy increases with chemical complexity and flexibility
- this only holds for substances in the same physical state
- the effect of physical state dominates the effect of molecular complexity
effect of temperature
as temperature increases, entropy increases
- higher temperature means more freedom of molecular motion
draw graph for temperature vs entropy
discontinuous jumps at phase changes
entropy change upon dissolution
- salt gains entropy as it is dispersed
- water loses entropy as it is ordered around the ions
- net entropy change depends on the relative magnitudes of entropy changes in both solute and solvent entropy