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The volumetric heat capacity can also be expressed as the specific heat capacity (heat capacity per unit of mass, in J⋅K −1 ⋅kg −1) times the density of the substance (in kg/L, or g/mL). [1] It is defined to serve as an intensive property .
Professionals in construction, civil engineering, chemical engineering, and other technical disciplines, especially in the United States, may use the so-called English Engineering units, that include the pound (lb = 0.45359237 kg) as the unit of mass, the degree Fahrenheit or Rankine ( 5 / 9 K, about 0.55556 K) as the unit of temperature ...
2 (736 J⋅K −1 ⋅kg −1) is greater than that of an hypothetical monatomic gas with the same molecular mass 28 (445 J⋅K −1 ⋅kg −1), by a factor of 5 / 3 . The vibrational and electronic degrees of freedom do not contribute significantly to the heat capacity in this case, due to the relatively large energy level gaps for both ...
Potential energy with respect to gravity, close to Earth, per unit mass: gh, where g is the acceleration due to gravity (standardized as ≈9.8 m/s 2) and h is the height above the reference level (giving J/kg when g is in m/s 2 and h is in m).
Within the human comfort range between 20 and 30 °C, some PCMs are very effective, storing over 200 kJ/kg of latent heat, as against a specific heat capacity of around one kJ/(kg*°C) for masonry. The storage density can therefore be 20 times greater than masonry per kg if a temperature swing of 10 °C is allowed. [ 2 ]
Temperature is a physical quantity that quantitatively expresses the attribute of hotness or coldness.Temperature is measured with a thermometer.It reflects the average kinetic energy of the vibrating and colliding atoms making up a substance.
Boltzmann constant: The Boltzmann constant, k, is one of seven fixed constants defining the International System of Units, the SI, with k = 1.380 649 x 10-23 J K-1.The Boltzmann constant is a proportionality constant between the quantities temperature (with unit kelvin) and energy (with unit joule).
Enthalpies of melting and boiling for pure elements versus temperatures of transition, demonstrating Trouton's rule. In thermodynamics, the enthalpy of fusion of a substance, also known as (latent) heat of fusion, is the change in its enthalpy resulting from providing energy, typically heat, to a specific quantity of the substance to change its state from a solid to a liquid, at constant pressure.