This document provides an introduction to fundamentals of thermodynamics. It defines key concepts such as systems, surroundings, boundaries, properties, and processes. It describes different types of systems including closed, open, and isolated systems. It also defines intensive and extensive properties, and explains thermodynamic equilibrium, states, paths, processes, cycles, and pure substances.

1. Fundamentals of
THERMODYNAMICS

2. Introduction
• Thermodynamics is science of energy transfer and its effects on properties.
• Main aim is to convert disorganized form of energy into organized form of
energy in an efficient manner.
• Based on the macroscopic approach which does not require knowledge of
behavior of individual particles and is called classical thermodynamics.

3. System, Surroundings, and Boundary
• A thermodynamic system is defined as quantity of matter or a region in space
chosen for study.
• The region outside the system is called surroundings.
• The real or imaginary surface that separates the system from its
surroundings is called boundary.
• Universe = System + Surroundings

4. Types of System
• Closed System
• Open System
• Isolated System

5. Closed System
• A closed system consists of fixed amount of mass and no mass may
cross the system boundary but energy in form of heat and work may
cross the system boundary.
• The closed system boundary may move.
• Examples of closed systems are sealed tanks and piston cylinder
devices without valves.

6. Open System or Control Volume
• An open system has mass as well as energy crossing the boundary, called a
control surface.
• Examples of open systems are pumps, compressors, turbines, valves and heat
exchangers.

7. Isolated system
• An isolated system is one in which there is no interaction between the
system and surroundings.
• It is of fixed mass and energy, and there is no mass or energy transfer across
the system boundary.
• Examples of isolated system are universe and hot coffee in a well insulated
flask.

8. Closed, Open, and Isolated Systems
Types of Energy Mass Transfer Examples
Closed System Yes No Gas in a sealed
container
Open System Yes Yes Turbines,
pumps, valves
etc.
Isolated System No No Universe,
Thermoflask

9. Properties of a System
• Any measurable characteristic of a system in equilibrium is called a
property.
• The property is independent of the path used to arrive at the system
condition.
• Properties are point functions.
• Properties are exact differentials.
• Properties may be intensive or extensive.

10. Extensive Properties
• Extensive properties depends on size or mass of the system.
• Some extensive properties are:
a. Mass
b. Volume
c. Total Energy
d. Electric Charge
e. Magnetization

11. Intensive Properties
• Intensive properties are independent of size or mass of the system.
• Some intensive properties are:
a. Pressure
b. Temperature
c. Density
d. Velocity
e. Viscosity

12. Important points w.r.t Properties
• Extensive properties per unit mass are intensive properties. For example, the
specific volume v, is defined as
v =
𝑉𝑜𝑙𝑢𝑚𝑒
𝑚𝑎𝑠𝑠
=
𝑉
𝑚
=
𝐸𝑥𝑡𝑒𝑛𝑠𝑖𝑣𝑒
𝐸𝑥𝑡𝑒𝑛𝑠𝑖𝑣𝑒
= Intensive
• Specific Properties are intensive properties.

13. Thermodynamics Equilibrium
A system is said to be in thermodynamic equilibrium if it maintains
a. Thermal Equilibrium ( Equality of Temperature )
b. Mechanical Equilibrium ( Equality of Forces / Pressure )
c. Chemical Equilibrium ( Equality of Chemical Potential )

14. State, Path, and Process
• Condition of a system as defined by properties of system is known as state of
a system.
• Series of state of system through which process occurs is known as path of a
system.
• Any change of state of a system is known as process.
• Some of the processes are-
Process Property held
constant
Isobaric Pressure
Isothermal Temperature
Isochoric Volume
Isentropic Entropy

15. Thermodynamic cycle
• A system is said to have undergone a cycle if the initial and final points are
same.
• Minimum number of processes required for a cycle are 2.
• For a cycle change in property is equal to zero.

16. Pure Substance
• A substance is said to be a pure substance if it is
a. Homogeneous in Chemical Composition.
b. Homogeneous in Chemical Aggregation.
• Examples of pure substance are atmospheric air, steam-water mixture and
combustion products of a fuel.
• Phase ( solid, liquid, gas ) is not considered while determining pure
substance.