Microscopic Approach:

• Internal energy: Imagine bouncing balls representing particles in a system, embodying their kinetic energy through movement and potential energy via their relative distance from each other.

• Temperature: Picture the balls’ average speed depicting the temperature. Faster balls moving with greater kinetic energy mean higher temperature.

• Specific heat capacity: Imagine adding energy to the balls, increasing their average kinetic energy. The varying levels of energy needed would represent the specific heat capacity of different systems.

• Thermal conductivity: Visualize heat transfer by balls continuously bouncing off each other, sharing their energy. Materials with efficiently transferred energy exhibit higher thermal conductivity.

• Thermal expansion: Think of the balls’ heightened activity and greater spacing upon gaining energy, causing the system’s volume to expand with rising temperature.

Macroscopic Approach:

• Heat: Imagine a flowing stream of water. Heat transfer is like a river of thermal energy moving between objects of distinct temperatures, akin to the movement of water downstream.

• Work: Visualize a piston pushing an object, resulting in energy transfer akin to the mechanical energy of a moving object.

• First law of thermodynamics: Picture a closed container with no openings. The principle states that the total energy inside remains the same, just like a sealed jar keeping its contents intact.

• Second law of thermodynamics: Imagine a room with messy toys. In time, the disorder (entropy) increases without effort. This law describes the universal tendency toward greater entropy.

• Ideal gas law: Imagine balloon filling with air, its pressure, volume, and temperature interconnected like variables in an equation.

• Adiabatic process: Picture a sealed vessel with no leaks. As energy moves within, no heat escapes or enters, like thermal energy isolated within a vacuum.