calorimetric , auch: calorimetrical

The above rules refer only to suitable calorimetric materials.

However, in a calorimetric experiment, the amount of heat given off or absorbed must be corrected for this effect.

All three of these enthalpies can be determined experimentally by calorimetric methods.

The calorimetric equipment to do this is fairly complicated and the measurements are labor-intensive.

The calibration of the calorimetric detectors is a key parameter and has to be performed very carefully.

From there, the dye is washed off with some type of solvent and measured using a calorimetric technique.

It is this quantity which is normally determined during calorimetric experiments (see below).

Again, simple algebraic manipulation is required; for example, calorimetric experiments give:

Empirically, it is convenient to measure properties of calorimetric materials under experimentally controlled conditions.

From this, further mathematical and thermodynamic reasoning leads to another relation between classical calorimetric quantities.

Then it can be shown that one can write a thermodynamic version of the above calorimetric rules:

A mathematical correction factor, known as the phi-factor, can be used to adjust the calorimetric result to account for these heat losses.

Here the classical rule is assumed to hold for the calorimetric material being used, and the propositions are mathematically written:

The corresponding thermopile of high thermal conductivity surrounds the experimental space within the calorimetric block.

Crystallinity can be measured using x-ray diffraction, but calorimetric techniques are also commonly used.

Onsager suggested that experimentalists look for a dramatic change in heat capacity by performing a careful calorimetric experiment.

Water evaporates, diffuses through the tube connecting two chambers of the calorimetric cell and is absorbed by the studied substance.

However, the experimentalists alluded to the fact, that calorimetric tests with 10-GeV electrons were executed already in 1969.

Thermochemical methods involve the calorimetric determination of the enthalpies of combustion, formation and other processes.

A sorption calorimetric experiment is performed at isothermal regime, but different temperatures can be studied in separate experiments.

Phelps criticized both the calorimetric techniques and the underlying theory described in the Phillips/Mills/Chen article.

In their publication, the investigators show details of their calorimeters' design and teach the technology of achieving high calorimetric accuracy.

The calorimetric method provides a quantitative thermodynamic scale of acetate properties by measuring the heat of adsorption.

The calorimetric constant will vary from instrument to instrument, and can be determined by analyzing a well-characterized sample with known enthalpies of transition.

Heats of formation can be determined experimentally though calorimetric studies; however, calculated enthalpies are more commonly used due to the greater ease of acquisition.