The document outlines the three laws of thermodynamics, explaining concepts such as energy conservation, entropy, and temperature relationships with entropy in crystals. It further categorizes chemical reactions into exothermic, endothermic, spontaneous, and non-spontaneous types, detailing how Gibbs energy influences their spontaneity. The document concludes with a discussion on reversible and non-reversible reactions, emphasizing the impact of temperature on the equilibrium state and thermochemistry.

1. Laws of
Thermodynamic
s
M U H A M M A D A H M A D ( L 1 F 2 0 B S P H 0 0 4 0 )

3. 1st Law
• The First Law of Thermodynamics states that energy can be converted from one form to another
with the interaction of heat, work and internal energy, but it cannot be created nor destroyed,
under any circumstances.
ΔU=q+w
• ΔU is the total change in internal energy of a system,
• q is the heat exchanged between a system and its surroundings, and
• w is the work done by or on the system.

4. • Work is also equal to the negative external pressure on the system multiplied by the change in
volume:
w=−pΔV
where P is the external pressure on the system, and ΔV is the change in volume. This is specifically
called "pressure-volume" work.
ΔUsystem=−ΔUsurroundings

5. 2nd Law
• The Second Law of Thermodynamics states that "in all energy exchanges, if no energy enters or
leaves the system, the potential energy of the state will always be less than that of the
initial state."
Eff=W=1−QcQhEff=WQh=1−QcQh
•This is also commonly
referred to as entropy.

6. Coefficient of Performance
EffC=1TcThEffC=1TcTh

7. 3rd Law
• The Third Law states,
“The entropy of a perfect crystal is zero when the temperature of the crystal is equal to
absolute zero (0 K).”
S – S0 = 𝑘B ln𝛀
• S is the entropy of the system.
• S0 is the initial entropy.
• 𝑘B denotes the Boltzmann constant.
• 𝛀 refers to the total number of microstates that are consistent with the system’s macroscopic
configuration.

8. CHEMICAL
REACTIONS
This Photo by Unknown author is licensed under CC BY.
Abdulhannan Mirza(L1F20BSPH0016)

9. CHEMICAL REACTION
The process through which substances convert into
other substances is known as a chemical reaction.
For example the formation of water from hydrogen
and oxygen:

10. CATEGORIES OF CHEMICAL
REACTION
Chemical reactions are of the following categories:
○Exothermic and Endothermic
○Spontaneous and Non-Spontaneous
○Reversible and Non-Reversible
On the basis heat evolution the two categories are,
Exothermic Reactions:
The chemical reactions which release energy during the process.
Endothermic Reactions:
The chemical reactions which absorb energy during the process.

11. SPONTANEOUS AND NON-
SPONTANEOUS REACTIONS
The propagation of a reaction determines whether it is spontaneous or
not:
Spontaneous Reactions:
If a reaction is capable of initiating or propagating on its own it is called
spontaneous.
Non-Spontaneous Reactions:
If a reaction is not capable of initiating or propagating on its own it is
called spontaneous.

12. SPONTANEOUS REACTIONS
These reactions have the following properties:
• They are exothermic.
• The reactants are at a higher energy level than products.
• There Gibbs energy is negative.

13. NON-SPONTANEOUS REACTIONS:
These reactions have the following properties:
• They are endothermic.
• The reactants are at a lower energy level than the products.
• There Gibbs energy is positive.

14. GIBBS ENERGY AND SPONTANEITY:
Gibbs Energy
The energy required to initiate a reaction is known as its Gibbs energy.
This energy determines the spontaneity of a reaction, since it tells
whether a reaction will absorb or release energy on initiations.

15. Gibbs energy of Spontaneous Reactions:
If the value of Gibbs energy for a reaction is negative, it means that it will
release energy on initiation and hence it will be spontaneous.
Gibbs energy of Non-Spontaneous Reactions:
If the value of Gibbs energy for a reaction is positive, it means that it will
absorb energy on initiation and hence it will be non-spontaneous.

16. Reversible and Non-
Reversible Reactions
Muhammad Uzair

17. REVERSIBLE & IRREVERSIBLE
A chemical reaction is the one in which a
substance converts into another, this is what is
known as a non-reversible reaction.
In some reactions the converted substance also
coverts back into the original substance, these are
known as reversible reaction.

18. PROPERTIES OF REVERSIBLE
REACTION:
• Two reactions forward and reverse take place
simultaneously.
• Forward reaction slows down over time while reverse
reaction speeds up.
• The end result of the reaction is Equilibrium state.

19. CHEMICAL EQUILIBRIUM:
• The point in a reversible reaction where the forward and reverse
reaction take place at the same rate.
• The number of reactants converting into products is equal to the
number of products converting into reactants.
• The reaction does not stop but appears to be stationary.
• Further product cannot be yielded without somehow disturbing
the equilibrium.

20. THERMOCHEMISTRY OF
REVERSIBLE
REACTIONS:
Thermochemistry deals with the heat energy absorbed or
released in a reaction. It studies the effect of temperature on
chemical reactions.
The equilibrium state can be affected by temperature and its
effect can be determined by thermochemistry.

21. EFFECT OF INCREASING
TEMPRATURE:
• Increasing the temperature causes heat to transfer from
surrounding to the system, which favours exothermic processes
while diminishes endothermic processes.
• If the forward reaction is exothermic the increasing temperature
increases the rate of it while the endothermic reverse reaction is
slowed, thus more product is formed.
• If the forward reaction is endothermic the increasing
temperature decreases the rate of it while the endothermic
reverse reaction speeds up, thus more reactant is formed.

22. EFFECT OF DECREASING
TEMPRATURE:
 Decreasing the temperature causes heat to transfer from the
system to the surrounding , which favours endothermic processes
while diminishes exothermic processes.
 If the forward reaction is endothermic the decreasing temperature
increases the rate of it while the exothermic reverse reaction is
slowed, thus more product is formed.
 If the forward reaction is exothermic the decreasing temperature
decreases the rate of it while the endothermic reverse reaction
speeds up, thus more reactant is formed.