Thermodynamics and Electrochemistry

Introduction to Thermodynamics

• Study of Energy: Energy can be transformed from one form to another. Energy cannot be created.
• Types of Energy: Solar, Nuclear, Thermal, Chemical, Mechanical, Electrical Energy.

Applications of Thermodynamics

• Useful in engineering and chemistry, such as refrigerators, nuclear plants.

System and Surroundings

• System: The focus of the study.
• Surroundings: The region outside the system.
• Boundary: Separates the system and surroundings.

Types of Thermodynamic Systems

• Open System: Exchange of heat and matter occurs.
• Closed System: Only heat exchange occurs.
• Isolated System: Neither heat nor matter exchange occurs.

Thermodynamic Processes

• Isothermal Process: Process at constant temperature.
• Isochoric Process: Process at constant volume.
• Isobaric Process: Process at constant pressure.
• Adiabatic Process: Process with no heat exchange.

Work and Heat Sign Convention

• Work Done on the System: Positive (compression)
• Work Done by the System: Negative (expansion)
• Heat Inward: Positive
• Heat Outward: Negative

Reversible and Irreversible Processes

• Reversible Process: Slowly, maintains equilibrium.
• Irreversible Process: Sudden, does not maintain equilibrium.

First Law of Thermodynamics

• Principle of energy conservation: Energy cannot be created or destroyed.
• Formula: ( \Delta U = Q + W )

Electrochemistry

• Standard Electrode Potential: Reduction potential of an electrode under standard conditions.
• Nernst Equation: ( E = E^0 - \frac{RT}{nF} \ln Q )
• Cell Reaction: Combination of oxidation and reduction.

Practical Questions

• Questions related to thermodynamics and electrochemistry like calorie to joule conversion, unit conversion.

These notes primarily summarize important topics related to thermodynamics and electrochemistry, which may be useful for your study and review.