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1 cal / °C⋅g = 1 Cal / °C⋅kg = 1 kcal / °C⋅kg = 4184 J / kg⋅K [20] = 4.184 kJ / kg⋅K . Note that while cal is 1 ⁄ 1000 of a Cal or kcal, it is also per gram instead of kilo gram : ergo, in either unit, the specific heat capacity of water is approximately 1.
The SI unit for heat capacity of an object is joule per kelvin (J/K or J⋅K −1). Since an increment of temperature of one degree Celsius is the same as an increment of one kelvin, that is the same unit as J/°C. The heat capacity of an object is an amount of energy divided by a temperature change, which has the dimension L 2 ⋅M⋅T −2 ...
The contribution of the muscle to the specific heat of the body is approximately 47%, and the contribution of the fat and skin is approximately 24%. The specific heat of tissues range from ~0.7 kJ · kg−1 · °C−1 for tooth (enamel) to 4.2 kJ · kg−1 · °C−1 for eye (sclera). [13]
Cal-th (kg-cal-th) Cal th: 1.0 ... (15°C) kcal-15 (g-cal-15) kcal 15: 1.0 kcal 15 (4.2 kJ) calorie (15°C) cal-15 (g-cal-15) cal 15: 1.0 ...
Energy density is thus commonly expressed in metric units of cal/g, kcal/g, J/g, kJ/g, MJ/kg, cal/mL, kcal/mL, J/mL, or kJ/mL. Energy density measures the energy released when the food is metabolized by a healthy organism when it ingests the food (see food energy for calculation).
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).
The SI unit of volumetric heat capacity is joule per kelvin per cubic meter, J⋅K −1 ⋅m −3. 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.
However, heating 0 °C ice to 20 °C requires additional energy to melt the ice. We can treat these two processes independently and using the specific heat capacity of water to be 4.18 J/(g⋅K); thus, to heat 1 kg of ice from 273.15 K to water at 293.15 K (0 °C to 20 °C) requires: (1) 333.55 J/g (heat of fusion of ice) = 333.55 kJ/kg = 333. ...