Chemical Thermodynamics
1. :
- Open systems: exchange energy and matter with surroundings
- Closed systems: exchange only energy
- Isolated systems: no exchange of energy or matter
2. :
- State functions: values depend on the state of the system, not the path taken to reach that state
- Path functions: values depend on the specific path taken to change the state
3. The :
- Energy is conserved within an isolated system
4. :
- H = U + PV; represents the total heat content of a system
5. :
- S = k ln W; measures the randomness or disorder in a system
6. The :
- The entropy of an isolated system always increases
7. :
- G = H - TS; a measure of the spontaneity and equilibrium of a system
8. Equilibrium:
- G = minimum; a system reaches equilibrium when the free energy is minimized
9. Chemical Reactions and Spontaneity:
- A chemical reaction is spontaneous if it lowers the free energy of the system (ΔG< 0)
10. Standard State:
- A reference state defined for temperature, pressure, and concentration
11. Gibbs Free Energy Change (ΔG°):
- ΔG° = ΔH° - TΔS°; predicts the spontaneity of a reaction at standard state
12. Reaction Quotient (Q):
- Q represents the ratio of product concentrations to reactant concentrations at any point in a reaction
13. Equilibrium Constant (K):
- K is the value of Q at equilibrium conditions
14. Le Chatelier’s Principle:
- When a system encounters stress, it shifts equilibrium to counteract the change
15. Partial Pressure:
- Pressure exerted by a specific gas in a mixture of gases
16. Raoult’s Law:
- PTotal = P1 + P2 + … + Pn; partial pressure of each component in a mixture is proportional to its mole fraction
17. Henry’s Law:
- The partial pressure of a gas above a solution is proportional to the concentration of the gas in the solution
18. Colligative Properties:
- Properties that depend on the concentration of particles in a solution
19. Boiling Point Elevation:
- The boiling point of a solution increases with increasing concentration of solute
20. Freezing Point Depression:
- The freezing point of a solution decreases with increasing concentration of solute
21. Osmotic Pressure:
- The pressure required to prevent the flow of solvent across a semipermeable membrane
22. Electrochemical Cells:
- Galvanic cells: spontaneous reactions produce electrical energy
- Electrolytic cells: electrical energy is used to drive nonspontaneous reactions
23. Standard Reduction Potential:
- Measure of the tendency of a half-reaction to undergo reduction
24. Nernst Equation:
- Relates the cell potential of an electrochemical cell to its standard reduction potential and the concentrations of reactants and products.
🧠 Smart Recommendations
Related Content
Based on your current topic, we recommend studying:
- Thermal Properties of Matter - Continue with heat transfer concepts
- Heat Engines and Refrigerators - Apply thermodynamics to real-world systems
- Chemical Equilibrium - Connect with chemical reaction dynamics
Students Also Studied
After completing this topic, students typically explore:
- Microscopic and Macroscopic Approach to Thermal Properties - For deeper understanding of kinetic theory
- Carnot Engine and Carnot Theorem - For advanced thermodynamic cycles
- Structure of the Atom - For atomic basis of thermal properties
Personalized Learning Path
- Foundational: Complete this chemical thermodynamics topic
- Next Level: Study thermal properties and heat transfer
- Advanced: Explore heat engines and efficiency calculations
- Application: Connect to chemical equilibrium and reactions
Quick Practice
🎯 NEET Focus Areas
- High Weightage: Laws of Thermodynamics (8-10 questions)
- Important: Entropy and Free Energy (6-8 questions)
- Key Concepts: State functions, enthalpy changes (5-7 questions)
- Applications: Chemical equilibrium and spontaneity (4-6 questions)
📋 Quick Reference
- First Law: ΔU = q + w (Energy conservation)
- Second Law: ΔS_universe ≥ 0 (Entropy increase)
- Gibbs Free Energy: ΔG = ΔH - TΔS (Spontaneity)
- Key Formula: ΔG° = -RT ln K (Equilibrium constant)
BETA
