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All values refer to 25 °C and to the thermodynamically stable standard state at that temperature unless noted. Values from CRC refer to "100 kPa (1 bar or 0.987 standard atmospheres)".
A calorimeter constant (denoted C cal) is a constant that quantifies the heat capacity of a calorimeter. [1] [2] It may be calculated by applying a known amount of heat to the calorimeter and measuring the calorimeter's corresponding change in temperature.
Chemical formula Δ f H ⦵ /(kJ/mol) Acetone: Liquid C 3 H 6 O: −248.4 Benzene: Liquid C 6 H 6: 48.95 Benzoic acid: Solid C 7 H 6 O 2: −385.2 Carbon tetrachloride: Liquid CCl 4: −135.4 Carbon tetrachloride: Gas CCl 4: −95.98 Ethanol: Liquid C 2 H 5 OH −277.0 Ethanol: Gas C 2 H 5 OH −235.3 Glucose: Solid C 6 H 12 O 6: −1271 ...
Vapor-pressure formula for ammonia: [4] log 10 P = A – B / (T − C), where P is pressure in kPa, and T is temperature in kelvins;
The centigrade heat unit (CHU) is the amount of heat required to raise the temperature of one pound (0.45 kg) of water by one Celsius degree. It is equal to 1.8 Btu or 1,899 joules. [26] In 1974, this unit was "still sometimes used" in the United Kingdom as an alternative to Btu. [27]
The Steinhart–Hart equation is a model relating the varying electrical resistance of a semiconductor to its varying temperatures.The equation is = + + (), where is the temperature (in kelvins),
When discussing the chemical energy contained, there are different types which can be quantified depending on the intended purpose. One is the theoretical total amount of thermodynamic work that can be derived from a system, at a given temperature and pressure imposed by the surroundings, called exergy.
Here is a similar formula from the 67th edition of the CRC handbook. Note that the form of this formula as given is a fit to the Clausius–Clapeyron equation, which is a good theoretical starting point for calculating saturation vapor pressures: log 10 (P) = −(0.05223)a/T + b, where P is in mmHg, T is in kelvins, a = 38324, and b = 8.8017.