Thermodynamics in Chemistry: Short Notes

Thermodynamics is a branch of physical chemistry concerned with the relationship between heat, work, temperature, and other forms of energy. It essentially deals with the transfer and transformation of energy in chemical and physical processes.

Thermodynamics — Chemistry Short Notes 📚

Here are some key concepts in thermodynamics for chemistry:

Thermodynamics in Chemistry — Systems and Surroundings

• Isolated system: No exchange of energy or matter with the surroundings.
• Closed system: Exchange of energy but not matter with the surroundings.
• Open system: Exchange of both energy and matter with the surroundings.

1. State functions: Properties of a system that depend only on its current state, not on how it got there (e.g., temperature, pressure, internal energy).
2. Path functions: Properties that depend on the specific path taken between two states (e.g., heat, work).

• Surroundings: Everything outside the system.

1. Zeroth law: If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.
2. First law: Energy cannot be created or destroyed, only transferred or transformed (ΔU = Q + W, where ΔU is the change in internal energy, Q is heat, and W is work).
3. Second law: The entropy of an isolated system never decreases over time. In simpler terms, disorder always increases in a closed system.
4. Third law: The entropy of a system approaches a constant minimum value as the temperature approaches absolute zero.

State Functions and Path Functions

1. Internal energy (U): Total energy of a system, including kinetic and potential energy of its molecules.
2. Enthalpy (H): U + PV (where P is pressure and V is volume).
3. Entropy (S): A measure of disorder in a system.
4. Free energy (G): G = H — TS. Determines the spontaneity of a process at constant temperature and pressure.

Laws of Thermodynamics:

1. Applies thermodynamic principles to chemical reactions.
2. Predicts spontaneity, feasibility, and equilibrium of reactions.
3. Explains factors like enthalpy change (ΔH), entropy change (ΔS), and Gibbs free energy change (ΔG) in chemical processes.

Thermodynamics — Chemistry Short Notes 📚

Thermodynamics — Chemistry Short Notes 📚

Thermodynamics — Chemistry Short Notes 📚

Thermodynamics — Chemistry Short Notes 📚

Thermodynamic Functions:

1. Internal energy (U): Total energy of a system, including kinetic and potential energy of its molecules.
2. Enthalpy (H): U + PV (where P is pressure and V is volume).
3. Entropy (S): A measure of disorder in a system.
4. Free energy (G): G = H — TS. Determines the spontaneity of a process at constant temperature and pressure.

Chemical Thermodynamics:

1. Applies thermodynamic principles to chemical reactions.
2. Predicts spontaneity, feasibility, and equilibrium of reactions.
3. Explains factors like enthalpy change (ΔH), entropy change (ΔS), and Gibbs free energy change (ΔG) in chemical processes.

Biological Classification Notes

Hormones Notes — The Tiny Messengers of Your Body

Error Notes — Expected Questions in NEET/JEE

Solutions Short Notes for NEET/JEE

Some Basic Concepts of Chemistry — Short Notes

Atomic Structure — Chemistry Short Notes

Periodic Table — Chemistry Short Notes

Chemical Elements and Formulas — Chemical Compounds with their Corresponding Names

Chemical Bonding — Chemistry Short Notes

Originally published at https://www.vhtc.org.