Thermodynamics — NEET Chemistry Concepts
Every Chemistry concept in Thermodynamics, explained around the doubts students actually search. Tap any concept for the full note with NCERT context and NEET traps.
- The Four Laws of Thermodynamics (Zeroth, First, Second, Third) Explained for NEET
- Macroscopic vs Microscopic View of a System in Thermodynamics
- Thermodynamic Equilibrium: Why Laws Apply Only at Equilibrium
- System, Surroundings, Boundary and the Universe in Thermodynamics
- Adiabatic Wall vs Diathermic Wall: Difference Explained Simply
- Why We Can Only Measure the Change in Internal Energy (ΔU), Not Absolute U
- Old vs New IUPAC Sign Convention for Work (Physics vs Chemistry)
- Joule's Paddle-Wheel Experiment: Why Adiabatic Work Is Path-Independent
- Difference Between Heat and Work as Energy Transfer
- Law of Conservation of Energy in Thermodynamics (First Law)
- Work Done in Single-Step vs Multi-Step (Stepwise) Compression
- Reversible Process in Thermodynamics: Definition, Meaning and Why It Is Infinitely Slow
- What Is an Irreversible Process in Thermodynamics?
- Work and Heat at Constant Volume (Isochoric): Why ΔU = qV
- Why qV = ΔU: Heat at Constant Volume Equals Internal Energy Change
- Why qP Equals Delta H (Heat at Constant Pressure)
- Why Enthalpy Is Defined as H = U + pV
- Deriving ΔH = ΔU + Δn_g RT (Enthalpy and Internal Energy Relation)
- What Does Δn_g Mean? (Gaseous Moles: Products Minus Reactants)
- When Is ΔH Equal to ΔU? (Solids, Liquids, and Δn_g = 0)
- Extensive Properties: Mass, Volume, Enthalpy, Heat Capacity Explained
- Intensive Properties in Thermodynamics: Temperature, Pressure, Density
- Extensive vs Intensive Properties: Difference with Examples (NEET)
- What Is a Molar Property? (Molar Volume and Molar Heat Capacity)
- What Is Heat Capacity (C)? Meaning, Formula and Units
- What Is Molar Heat Capacity (Cm)? Definition, Formula and Units
- What Is Specific Heat Capacity? Meaning, Formula and Units (NEET)
- Difference Between Cp and Cv (Heat Capacity at Constant Pressure vs Constant Volume)
- Deriving Cp - Cv = R for an Ideal Gas (Mayer's Relation)
- What Is Calorimetry? Measuring Heat Changes (NEET Class 11)
- Bomb Calorimeter: How It Measures ΔU at Constant Volume
- Constant-Pressure Calorimeter: How to Measure ΔH
- Heat Lost by Reaction = Heat Gained by Calorimeter (Calorimetry)
- Reaction Enthalpy = Enthalpy of Products − Enthalpy of Reactants
- Standard Enthalpy of Reaction and the Standard State (1 bar)
- Standard State of a Substance: Meaning, 1 bar and 298 K (NEET)
- Standard Enthalpy of Fusion (Melting): Meaning, Sign and Value
- Standard Enthalpy of Vaporization: Meaning, Sign and Value
- Standard Enthalpy of Sublimation (ΔsubH°): NEET Notes
- Why Fusion, Vaporization and Sublimation Enthalpies Are Always Positive
- Reference State of an Element (Most Stable Form) Explained
- Why Standard Enthalpy of Formation of an Element Is Zero
- Difference Between Enthalpy of Formation and Reaction Enthalpy
- Thermochemical Equations: Rules and Conventions Explained
- Reversing and Multiplying Thermochemical Equations: How ΔH Changes
- Standard Enthalpy of Combustion (ΔcH°): Meaning, Sign and NEET Tricks
- Enthalpy of Atomization: Meaning, Formula and NEET Examples
- Bond Dissociation Enthalpy vs Mean Bond Enthalpy (Simple NEET Explanation)
- Why Successive C–H Bond Energies in Methane Differ (Even Though All 4 Bonds Are the Same)
- Enthalpy of Solution (Δsol H): Meaning, Formula and NEET Concept
- Enthalpy of Hydration of Ions: Meaning, Sign and NEET Uses
- Enthalpy of Solution = Lattice Enthalpy + Hydration Enthalpy
- Why Are Many Fluorides Less Soluble Than Chlorides? (Lattice Enthalpy)
- Enthalpy of Dilution: Meaning, Formula and Examples for NEET
- Ionization Enthalpy vs Ionization Energy (and Electron Gain Enthalpy vs Electron Affinity)
- What Is a Spontaneous Process in Thermodynamics?
- Spontaneity Does Not Mean Fast: The H2 + O2 Example (NEET Thermodynamics)
- Is Decrease in Enthalpy a Criterion for Spontaneity?
- Entropy as a Measure of Disorder or Randomness (NEET Thermodynamics)
- Entropy Order: Why Solid < Liquid < Gas
- What is Thermodynamics? System, Surroundings and Boundary Explained
- Open, Closed and Isolated Systems: Difference with Examples
- State Functions vs Path Functions: The Difference (with Examples)
- Isothermal, Adiabatic, Isobaric and Isochoric Processes
- What is Internal Energy (U) and Why is it a State Function?
- Heat and Work: IUPAC Sign Conventions Made Simple
- First Law of Thermodynamics: What ΔU = q + w Really Means
- Pressure-Volume Work: Work Done When a Gas Expands
- Reversible vs Irreversible Expansion: Why Maximum Work is Reversible
- Free Expansion of an Ideal Gas: Why Work and ΔU Are Zero
- Adiabatic vs Isothermal Expansion: Work Done on a p-V Curve
- What is Enthalpy (H)? Heat at Constant Pressure Explained
- Relation Between ΔH and ΔU: ΔH = ΔU + ΔngRT
- Exothermic vs Endothermic Reactions: Sign of ΔH and Energy Profiles
- Standard Enthalpy of Formation and Enthalpy of Reaction
- Hess's Law: How to Add Reactions to Find Unknown Enthalpy
- Bond Enthalpy: Calculating ΔH of a Reaction from Bond Energies
- Born-Haber Cycle and Lattice Enthalpy Explained
- Entropy (S) and the Second Law of Thermodynamics: Disorder Explained
- How to Predict the Sign of Entropy Change (ΔS) in a Reaction
- What Makes a Process Spontaneous? The Gibbs Energy Criterion
- Gibbs Free Energy (ΔG = ΔH − TΔS): How to Predict If a Reaction is Spontaneous
- Effect of Temperature on Spontaneity: Sign of ΔH and ΔS
- Gibbs Energy and Equilibrium: ΔG° = −RT ln K
- Gibbs Energy and Cell EMF: ΔG° = −nFE°cell Explained