Spontaneity.........................pptx

CsNHS Senior High School
Caestebanan National High School
MELCS
Predict the spontaneity of a process based on entropy.
(STEM_GC11CTIVa-b-140)
Explain the second law of thermodynamics and its
significance. (STEM_GC11CTIVa-b-142)
Use Gibbs’ free energy to determine the direction of a
reaction. (STEM_GC11CTIVa-b-143)

First Law of Thermodynamics
Energy cannot be created nor destroyed. Therefore, the
total energy of the universe is a constant.
Energy can, however, be converted from one form to
another or transferred from a system to the surroundings or
vice versa.

Spontaneous Process
Refers to processes that
occurs naturally

Spontaneous Process
Spontaneous processes
are those that can proceed
without any outside
intervention.

Spontaneous Process
Processes that are
spontaneous in one
direction are
nonspontaneous in the
reverse direction.

Spontaneous Process
 Processes that are spontaneous at one temperature may
be nonspontaneous at other temperatures.
 Above 0C it is spontaneous for ice to melt.
 Below 0C the reverse process is spontaneous.

Reversible Process
 In a reversible process the system
changes in such a way that the system
and surroundings can be put back in
their original states by exactly
reversing the process.
 Changes are infinitesimally small in a
reversible process

Reversible Process
 Irreversible processes cannot be undone by exactly
reversing the change to the system.
 All Spontaneous processes are irreversible.
 All Real processes are irreversible.

Entropy (S)
 a term coined by Rudolph Clausius in the 19th century.
 Clausius was convinced of the significance of the ratio
of heat delivered and the temperature at which it is
delivered,
𝑞
𝑇
 Therefore,
S = Sfinal  Sinitial

Entropy (S)
For a process occurring at constant temperature (an
isothermal process):
• qrev = the heat that is transferred when the process is carried out
reversibly at a constant temperature.
• T = temperature in Kelvin.

Secodn Law of Thermodynamics
 The entropy of the universe does not change for reversible
processes and increases for spontaneous processes.
• Reversible (ideal):
• Irreversible (real, spontaneous):

Entropy on the Molecular Scale
• Ludwig Boltzmann described the concept of entropy on the
molecular level.
• Temperature is a measure of the average kinetic energy of the
molecules in a sample.

1. Translational: Movement of the entire molecule from
one place to another.
2. Vibrational: Periodic motion of atoms within a
molecule.
3. Rotational: Rotation of the molecule on about an axis
or rotation about  bonds.

• Each thermodynamic state has a specific number of
microstates, W, associated with it.
• Entropy is
S = k lnW

•more particles
-> more states
•higher T
-> more entropy
-> more energy states -> more entropy
•less structure (gas vs solid)
-> more states -> more entropy

• The number of microstates and, therefore, the entropy
tends to increase with increases in
Temperature.
Volume (gases).
The number of independently moving molecules.

• Entropy increases with the
freedom of motion of molecules.
• Therefore,
S(g) > S(l) > S(s)

Dissolution of a solid:
Ions have more entropy (more states)
But,
Some water molecules have less
entropy (they are grouped around
ions).

Entropy Changes
• In general, entropy increases when
Gases are formed from liquids and
solids.
Liquids or solutions are formed from
solids.
The number of gas molecules
increases.
The number of moles increases.

Standard Entropies of Selected Substances at 298 K

Standard Entropies

Standard Entropies
S° for each component is found in a table.
Note for pure elements:

Entropy Changes in Surroundings
• Heat that flows into or out of the system also changes the
entropy of the surroundings.
• For an isothermal process:

For water:
• Hfusion = 6 kJ/mol
• Hvap = 41 kJ/mol
Ssurr = –Ssys

Entropy

Trends in Entropy
• Entropy for gas phase is greater than that of liquid or solid
of same substance
I2 (g) has greater entropy than I2 (s)
• More complex structures have greater entropy
C2H6 (g) has greater entropy than CH4 (g)
• Allotropes - more ordered forms have lower entropy
Diamond has lower entropy than graphite

Entropy Changes in System
S
rxn = nS
products  mS
reactants

Entropy
Calculate the standard entropy change for the following
using the table of standard values. (first, predict the sign for
S qualitatively)
2NH3(g)  N2(g) + 3H2(g)
nS
products

Entropy
2NH3(g)  N2(g) + 3H2(g)
S = nS
rxn products
 mS
reactants
= [(1)(191.5 J/K · mol) + (3)(131.0 J/K · mol)] - [(2)(193.0 J/K.mol)]
= 584.5 J/K · mol - 386 J/K · mol
S = 198.5 J/K · mol (Entropy increases)
rxn
(2 mol gas  4 mol gas)

Spontaneity.........................pptx

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