Thermodynamics and Heat Transfer

Flashcards covering key vocabulary and concepts related to thermodynamics, including definitions and examples.

Thermal Energy

The transfer of energy as heat accompanying both chemical and physical change.

1st Law of Thermodynamics

Energy cannot be created or destroyed, but it can be transferred.

Heat (q)

The thermal energy transferred from an object of higher temperature to an object of lower temperature.

Joules (J)

A unit of heat/energy; 1000 J = 1 kJ.

Calorie (cal)

A unit of heat/energy, defined as the amount of energy needed to raise the temperature of 1 gram of water by 1°C.

Specific Heat (c)

The amount of energy required to change the temperature of 1 gram of a substance by 1°C or 1 K.

Specific Heat Capacity

The value used to calculate heat capacity, dependent on mass, specific heat, and changes in temperature.

Exothermic Process

A process that releases energy, indicated by a negative change in thermal energy (q = -).

Endothermic Process

A process that absorbs energy, indicated by a positive change in thermal energy (q = +).

Heat Capacity Formula

q = mcΔT where q is heat transfer, m is mass, c is specific heat, and ΔT is the change in temperature.

Example of Thermal Energy Calculation

For a 200 kg wooden block with a specific heat of 1700 kg.°C, warming from 15°C to 25°C, the change in thermal energy is 340,000 J.