The zeroth law of thermodynamics states that if two systems are each in thermal equilibrium with a third, they are in thermal equilibrium with each other.Thermodynamics begins with the zeroth law because it was recognized later than the first and second, but turned out to be more fundamental. It was formulated by Ralph Fowler in 1931. The essence: thermal equilibrium is transitive. If coffee in a thermos and the air in the room have the same temperature, and the air in the room has the same as a book on the shelf, then the coffee and the book also 'agree' on temperature.
Although the idea of temperature is as ancient as observations of cooling, the formalization of the law occurred in the 20th century. Ralph Fowler in 1931, while discussing the principles of statistical mechanics, called this postulate 'zeroth' because it logically precedes the first and second laws, formulated earlier. The term quickly caught on.
The law underlies all thermometry and calorimetry. Without it, the concept of temperature would be undefined. Limits of applicability: the law holds for macroscopic systems in equilibrium. In non-equilibrium processes, for nanoscale objects, or in strong gravitational fields, refinements may be needed.
A thermometer works precisely because it reaches equilibrium with the object being measured, and we read the common temperature.
Thermometers appeared long before formal thermodynamics. Galileo created a thermoscope as early as 1593, not knowing that it embodied the zeroth law.
| N | variable | null depth ratio — null depth ratio |
| I_min | variable | minimum intensity — intensity watt per square metre |
| I_max | variable | maximum intensity — intensity watt per square metre |











