In everyday conversation, people use the words 'Heat' and 'Temperature' to mean the exact same thing (e.g., 'The heat of the sun' vs 'The temperature of the sun'). However, in strict Physics and Thermodynamics, these are two vastly different concepts.
Heat: A form of energy that flows between two bodies.
Temperature: A measurement of the degree of hotness or coldness.
Mass Dependency: Heat depends heavily on the mass/size of the object. Temperature does not.
SI Unit of Heat: Joule (J).
SI Unit of Temperature: Kelvin (K).
Measurement Tools: Heat is measured using a Calorimeter; Temperature is measured using a Thermometer.
Heat is a form of Energy. Specifically, it is the total kinetic energy of all the vibrating atoms inside an object. Because heat is actual physical energy transferring from a hot object to a cold object, it depends on the size and mass of the object. A massive ocean of cold water actually contains more total 'Heat Energy' than a tiny cup of boiling tea simply because the ocean has trillions of more vibrating water molecules.
Temperature is a Measurement. It is not energy itself. Instead, it is a measurement of the average kinetic energy of the molecules. It tells us the physical state or the degree of 'hotness' or 'coldness' of a body. Temperature does NOT depend on mass or size. A tiny cup of boiling water and a massive tank of boiling water both have the exact same temperature (100°C).
Heat is the total thermal energy contained inside an object, while Temperature is simply a numerical measurement of how hot or cold that object is.
The SI unit of Heat is the Joule (J), and the SI unit of Temperature is Kelvin (K).
No, temperature is independent of mass. A single drop of boiling water has the exact same temperature (100°C) as a massive bucket of boiling water.
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