For historical reasons, two main definitions of calorie are in wide use. The small calorie or gram calorie (usually denoted cal) is the amount of heat energy needed to raise the temperature of one gram of water by one degree Celsius (or one kelvin).  The large calorie, food calorie, or kilocalorie (Cal, calorie or kcal) is the amount of heat needed to cause the same increase in one kilogram of water. Thus, 1 kilocalorie (kcal) = 1000 calories (cal). By convention in food science, the large calorie is commonly called Calorie (with a capital C by some authors to distinguish from the smaller unit). In most countries, labels of industrialized food products are required to indicate the nutritional energy value in (kilo or large) calories per serving or per weight.
Calorie relates directly to the metric system, and therefore to the SI system. It is regarded as obsolete within the scientific community, since the adoption of the SI system, but is still in some use. The SI unit of energy is the joule, with symbol "J": one calorie (small) is defined as exactly 4.184 J; one kilocalorie (large) is 4184 J.
The calorie was first introduced by Nicolas Clément, as a unit of heat energy, in lectures during the years 1819–1824. This was the "large" calorie, viz. modern kilocalorie. The term entered French and English dictionaries between 1841 and 1867. It comes from Latin calor 'heat'.
The "small" calorie (modern calorie) was introduced by Pierre Antoine Favre (Chemist) and Johann T. Silbermann (Physicist) in 1852. In 1879, Marcellin Berthelot distinguished between gram-calorie (modern calorie) and kilogram-calorie (modern kilocalorie). Berthelot also introduced the convention of capitalizing the kilogram-calorie, as Calorie.
The modern calorie (cal) was first recognized as a unit of the cm-g-s system (cgs) in 1896, alongside the already-existing cgs unit of energy, the erg (first suggested by Clausius in 1864, under the name ergon, and officially adopted in 1882).
Already in 1928 there were serious complaints about the possible confusion arising from the two main definitions of the calorie and whether the notion of using the capital letter to distinguish them was sound. Use of the calorie was officially deprecated by the ninth General Conference on Weights and Measures, in 1948.
The alternate spelling calory is archaic.
The modern (small) calorie is defined as the amount of energy needed to increase the temperature of 1 gram of water by 1 °C (or 1 K, which is the same increment). The definition depends on the atmospheric pressure and the starting temperature. Accordingly, several different precise definitions of the calorie have been used.
|Name||Symbol||Conversions||Definition and notes|
? ? ?
|The amount of energy equal to exactly 4.184 J (Joules) and 1 kJ = 0.239 kcal.(a).|
|4 °C calorie||cal4||? 4.204 J
? ? 1.168×10-6 kW?h ? 2.624×1019 eV
|The amount of energy required to warm one gram of air-free water from 3.5 to 4.5 °C at standard atmospheric pressure. (c)|
|15 °C calorie||cal15||? 4.1855 J
? ? 1.1626×10-6 kW?h ? 2.6124×1019 eV
|The amount of energy required to warm one gram of air-free water from 14.5 to 15.5 °C at standard atmospheric pressure. (c) Experimental values of this calorie ranged from 4.1852 to 4.1858 J. The CIPM in 1950 published a mean experimental value of 4.1855 J, noting an uncertainty of 0.0005 J.|
|20 °C calorie||cal20||? 4.182 J
? ? 1.162×10-6 kW?h ? 2.610×1019 eV
|The amount of energy required to warm one gram of air-free water from 19.5 to 20.5 °C at standard atmospheric pressure. (c)|
|Mean calorie||calmean||? 4.190 J
? ? 1.164×10-6 kW?h ? 2.615×1019 eV
|Defined as of the amount of energy required to warm one gram of air-free water from 0 to 100 °C at standard atmospheric pressure. (c)|
|International Steam table calorie (1929)||? 4.1868 J
? ? 1.1630×10-6 kW?h ? 2.6132×1019 eV
|Defined as "international" watt hours = "international" joules exactly. (b)|
|International Steam Table calorie (1956)||calIT||? 4.1868 J
? = 1.1630×10-6 kW?h ? 2.6132×1019 eV
|Defined as 1.163 mW?h = 4.1868 J exactly. This definition was adopted by the Fifth International Conference on Properties of Steam (London, July 1956).|
The two definitions most common in older literature appear to be the 15 °C calorie and the thermochemical calorie. Until 1948, the latter was defined as 4.1833 international joules; the current standard of 4.184 J was chosen to have the new thermochemical calorie represent the same quantity of energy as before.
In a nutritional context, the kilojoule (kJ) is the SI unit of food energy, although the calorie is commonly used. The word calorie is commonly used with the number of kilocalories (kcal) of nutritional energy measured.
In the United States, most nutritionists prefer the unit kilocalorie to the unit kilojoules, whereas most physiologists prefer to use kilojoules. In the majority of other countries, nutritionists prefer the kilojoule to the kilocalorie. US food labelling laws require the use of kilocalories (under the name of "Calories"); kilojoules are permitted to be included on food labels alongside kilocalories, but most food labels do not do so. In Australia, kilojoules are officially preferred over kilocalories, but kilocalories retain some degree of popular use. Australian and New Zealand food labelling laws require the use of kilojoules; kilocalories are allowed to be included on labels in addition to kilojoules, but are not required. EU food labelling laws require both kilojoules and kilocalories on all nutritional labels, with the kilojoules listed first.
To facilitate comparison, specific energy or energy density figures are often quoted as "calories per serving" or "kcal per 100 g". A nutritional requirement or consumption is often expressed in calories or kilocalories per day.
Food nutrients as fat (lipids) contains 9 kilocalories per gram (kcal/g), while carbohydrate (sugar) or protein contains approximately 4 kcal/g. Alcohol in food contains 7 kcal/g. Food nutrients are also often quoted "per 100 g".
In other scientific contexts, the term calorie almost always refers to the small calorie. Even though it is not an SI unit, it is still used in chemistry. For example, the energy released in a chemical reaction per mole of reagent is occasionally expressed in kilocalories per mole. Typically, this use was largely due to the ease with which it could be calculated in laboratory reactions, especially in aqueous solution: a volume of reagent dissolved in water forming a solution, with concentration expressed in moles per litre (1 litre weighing 1 kilogram), will induce a temperature change in degrees Celsius in the total volume of water solvent, and these quantities (volume, molar concentration and temperature change) can then be used to calculate energy per mole. It is also occasionally used to specify energy quantities that relate to reaction energy, such as enthalpy of formation and the size of activation barriers. However, its use is being superseded by the SI unit, the joule, and multiples thereof such as the kilojoule.
In the past, a bomb calorimeter was used to determine the energy content of food by burning a sample and measuring a temperature change in the surrounding water. Today, this method is not commonly used in the United States and has been replaced by calculating the energy content indirectly from adding up the energy provided by energy-containing nutrients of food (such as protein, carbohydrates, and fats). The fibre content is also subtracted to account for the fact that fibre is not digested by the body.
both the IT calorie and the thermochemical calorie are completely independent of the heat capacity of water.