Thermal Energy and Temperature Concepts

These flashcards cover fundamental concepts related to temperature, thermal energy, kinetic energy, specific heat, and thermodynamic systems.

What are the units used for measuring temperature?

Celsius, Kelvin, and Fahrenheit.

What does thermal energy depend on?

It depends on how much material you have and is associated with the motion of particles.

How does temperature relate to kinetic energy?

Temperature is a measure of average kinetic energy; as temperature increases, kinetic energy increases.

Why do gas particles move with different velocities at a given temperature?

Gas particles have different amounts of energy transferred to them when they interact, resulting in a range of speeds.

What is the Boltzmann constant, Kb?

It is a constant used in statistical mechanics relating temperature to the kinetic energy of particles.

How is specific heat capacity affected by molecular-level structure?

The specific heat capacity is influenced by the presence and strength of intermolecular forces (IMFs).

What is the difference between open, closed, and isolated systems?

Open systems can transfer energy and matter; closed systems transfer energy but not matter; isolated systems do not transfer energy or matter.

What are state functions and path functions?

State functions describe the state of a system regardless of the process taken, while path functions depend on the specific process used to change the system's state.

What happens to thermal energy during an exothermic process?

Thermal energy flows out of the system, resulting in a negative change in enthalpy (ΔH).

What occurs during a phase change in terms of thermal energy?

Thermal energy flows from the surroundings to the system, making the process endothermic.