Question

Why do you not come to thermal equilibrium on a cold day

Answer 1

On a cold day, thermal equilibrium is not reached because the surrounding environment is colder than our body temperature. Heat transfer occurs from our body to the colder environment until a point of equilibrium is reached.

Step-by-step explanation:

On a cold day, thermal equilibrium is not reached because the surrounding environment is colder than our body temperature. In thermal equilibrium, there is no net heat transfer between two objects. However, on a cold day, our bodies lose heat to the colder environment, and the heat transfer continues until our body temperature drops and reaches a point of equilibrium.

For example, imagine stepping outside on a cold day without wearing a jacket. The air around you is colder than your body temperature, so heat transfers from your body to the air, resulting in a sensation of feeling cold. This process continues until your body and the environment reach a point of thermal equilibrium.

Answer 2

Two physical systems are in thermal equilibrium if no heat flows between them when they are connected by a path permeable to heat. Thermal equilibrium obeys the zeroth law of thermodynamics. A system is said to be in thermal equilibrium with itself if the temperature within the system is spatially and temporally uniform.

Systems in thermodynamic equilibrium are always in thermal equilibrium, but the converse is not always true. If the connection between the systems allows transfer of energy as heat but does not allow transfer of matter or transfer of energy as work, the two systems may reach thermal equilibrium without reaching thermodynamic equilibrium.