Lecture 1:

Lecture 1:

Introduction to Thermodynamics – Role of thermodynamic Principles in real-life situations – active learning and attitude of a true student – Course Outline – Syllabus

System, Definition and Types of Systems – Closed, Open, Isolated; System properties

Lecture 2:

Postulates of Thermodynamics:

(n+2) rule
Existence of stable equilibrium

Definitions of:

State
Point and Path Functions
Work

Deriving expression for Work from first principles (force balance)
Adiabatic work interactions (most direct path from one point to another)
Postulate III of Thermodynamics: Change of state is possible in at least one route and the adiabatic work is identified from the corresponding end states

Lecture 3:

Definition of Heat
Postulate IV of Thermodynamics or Zeroth Law of Thermodynamics: A&B are in equilibrium; B&C are in equilibrium, then A&C are in equilibrium
First law of Thermodynamics: dQ = dU + dW; importance of sign conventions
First law as applied to closed systems
Ideal gas concept – applied to gases; Enthalpy, Internal Energy and relation between the heat capacities of gases

Lecture 4:

First law as applied to open systems
Work refinements – Types of Work: Electrical, Mechanical, Surface Tension, Elastic, Kinetic Energy, Rotational Relativistic
Additional Enthalpies

Sensible Heat
Latent Heat: -Change of Phase, Chemical Reaction, Nuclear Reaction

Lecture 5:

Flow Systems:

Force balance on steady-state, steady flow systems

Isothermal Expansion
Converging Nozzle
Heat Exchanger
Adiabatic periodic piston
Ideal isothermal turbine
Ideal adiabatic turbine

Lecture 7:

Work – Energy cycles with examples – Flow Systems – Batch systems – Bernoulli equation as a special case of 1^st law of thermodynamics

;

Ideal Isothermal Turbine

The difference in the work produced in an adiabatic batch vs. flow system is related to the difference in D H & D U = D (PV)

= -nC_p (T₂-T₁)

Example 4: Adiabatic Expansion @ Constant Volume

For P >> P_intial; T à g T_e

Lecture 8:

Definition of Path Function

Part II of Example 4 – Constant Adiabatic Expansion @ Constant Pressure

Example 8 – Home Work problem 2.32: Real Gas work: Isothermal batch systems – Home Work Problem 2.29: ; H₂-H₁ = (v₁²-v₂²)/2

Lecture 9:

Historical approach to the second law of thermodynamics – Carnot (heat engine) and Clausius (entropy)

Examples demonstrating the Entropy phenomena, Concept of Equilibrium, Heat and Work

Definition of Reversible process – Rankine cycle

Concept of Thermodynamic Temperature

Lecture 10:

Definition of Thermodynamic Efficiency (h ) and its derivation

Introduction to Entropy – Definition, Concept of Entropy from heat engines

For any isolated system D S_system ³ 0;

For any system D S_system+D S_{surroundings ³}0

Homework Problems: 5.5, 5.8, 5.14

Entropy and 2^nd law of Thermodynamics – Definition and derivation of thermodynamic efficiency – Efficiency limits – functionality

Carnot Cycle: Definition and derivation of Carnot efficiency

Clausius’ Theorem: Any process can be broken into equivalent adiabatic and isothermal steps

For a process with less than a complete cycle, entropy is defined as:

Entropy is a state function; Entropy of the Universe is never conserved

Lecture 11:

Combined 1^st and 2^nd law of Thermodynamics: Conservation of Energy with respect to Entropy

Ideal gases and 2^nd law of Thermodynamics: Isochoric process, Isobaric Processes, Isothermal processes, Processes from (P₁, V₁, T₁) to (P₂, V₂, T₂) – with respect to Entropy and Adiabatic reversible processes: Isentropic processes

(n+2) rule for a single phase system with respect to Entropy

Examples of Second law of Thermodynamics, Reversible work, to calculate change in Entropy: Bird problem, Hilsch tube etc.