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- Topic tree
- Terms, Defintions and Symbols
- Concepts
- Infographics
- Problems and Solutions
- Board Level Unit test
- NEET / JEE Test
1. Topic tree
Unit 6: Thermodynamics
1. Introduction
- Overview of energy transformations
- Relevance to chemical reactions and physical processes
2. Thermodynamic Terms
- System and surroundings
- Types of systems: Open, closed, isolated
- State of the system
3. Internal Energy
- Definition and significance
- Work and heat exchange
- Internal Energy MCQ
4. First Law of Thermodynamics
- Statement and mathematical form
- Energy conservation principles
- Applications in chemical systems
5. Enthalpy (H)
- Definition and state function
- Relationship between ΔU\Delta U and ΔH\Delta H
6. Standard Enthalpy Changes
- Standard states
- Measurement and calculation
7. Enthalpy for Reactions
- Hess’s Law
- Applications and examples
8. Properties of Thermodynamic Quantities
- Extensive vs. Intensive Properties
9. Spontaneity and Processes
- Spontaneous and non-spontaneous processes
- Role of entropy in spontaneity
10. Second Law of Thermodynamics
- Entropy and its significance
11. Gibbs Free Energy (G)
- Definition and relationship to spontaneity
- Relation to equilibrium constants
12. Applications
- Predicting feasibility of reactions
- Driving forces in chemical changes
2. Terms, Definitions and Symbols
| Terms | Definitions |
| System-surroundings | A concept describing a system interacting with its surroundings. |
| Open-system | A system allowing the exchange of matter and energy with surroundings. |
| Closed-system | A system allowing only energy exchange, not matter. |
| Isolated-system | A system with no exchange of matter or energy. |
| State-function | A property depending only on the current state, not the path taken. |
| Internal-energy | Total energy contained in a system, including kinetic and potential energy. |
| Enthalpy-change | Heat exchange at constant pressure during a reaction. |
| Standard-state | Reference condition for thermodynamic measurements. |
| Hess’s-law | A law stating total enthalpy change is independent of the reaction path. |
| Energy-conservation | Principle that energy cannot be created or destroyed. |
| Heat-work | Two primary modes of energy transfer in a system. |
| State-properties | Properties defining the macroscopic state of a system. |
| Extensive-property | Property depending on the size/extent of the system. |
| Intensive-property | Property independent of the size of the system. |
| Thermodynamic-equilibrium | Condition where macroscopic properties remain constant over time. |
| Entropy-change | Measure of disorder or randomness in a system. |
| Gibbs-free-energy | Energy available to do work in a system at constant temperature and pressure. |
| Spontaneous-process | Process occurring without external energy input. |
| Non-spontaneous | A process requiring external energy input to occur. |
| Thermodynamic-reversibility | A process that can reverse with no net energy change. |
| Enthalpy-formation | Change in enthalpy when one mole of a compound forms. |
| Enthalpy-combustion | Change in enthalpy when one mole of substance combusts completely. |
| Entropy-increase | General tendency of entropy to increase in isolated systems. |
| Equilibrium-constant | Constant characterizing equilibrium concentrations of products and reactants. |
| Temperature-dependence | Dependence of reaction feasibility on temperature. |
| Chemical-potential | Energy driving chemical reactions towards equilibrium. |
| Phase-transition | Change between solid, liquid, and gaseous states of matter. |
| Energy-transfer | Exchange of energy between a system and its surroundings. |
| Reversible-process | Idealized process occurring infinitely slowly, maintaining equilibrium. |
| Irreversible-process | Process occurring spontaneously, creating entropy. |
3. Concepts
- Internal Energy
- Thermodynamics Lecture -1
Heat and Thermodynamics – Topic tree for class 11 State board
Thermodynamics Lecture part-2
Thermodynamics Lecture part-3
Thermodynamics Lecture part-4
Bomb Calorimeter
Physics of Refregerator
Termperature conversion
Liquefaction of Gases
Meyer’s equation
Carnot’s cycle
Gibb’s Free Energy
