Examples of 'enthalpies' in a sentence
Meaning of "enthalpies"
enthalpy (noun): Enthalpy is a thermodynamic property that describes the total heat content of a system
Show more definitions
- plural of enthalpy
How to use "enthalpies" in a sentence
Basic
Advanced
enthalpies
This is true for all enthalpies of formation.
Calculated enthalpies of formation are presentd for a number of cycloalkanes.
This curve can be used to calculate enthalpies of transitions.
Measurement of enthalpies of high temperature intermetallic compounds.
Uncertainties in derived enthalpies are assessed.
Enthalpies and free energies of mixing.
We will be looking at the molar enthalpies of fusion and vaporization.
Enthalpies of formation are not measured.
Reaction temperatures and enthalpies.
No melting enthalpies or spinning properties are mentioned.
Of reaction enthalpies.
The enthalpies of mixing were determined using a flow calorimetric technique.
The initial and final temperatures are determined based on enthalpies of the two feedstocks.
Add up the enthalpies of formation of the reagents of the reaction.
This allows incompatibilities to be recognized through low enthalpies of fusión and melting temperatures.
See also
Enthalpies of transfer from vapor to each solvent have been calculated.
These values correlate well with the enthalpies of complex formation with boron trifluoride.
Enthalpies of transfer from water to aqueous urea solutions are reported.
Covalent compounds usually have lower enthalpies of fusion and vaporization than ionic compounds.
Enthalpies of decomposition were calculated.
These temperatures and their associated enthalpies of transition depend on the source of the polypropylene.
Enthalpies of dissolution of the adducts in ethanol or methanol have been measured calorimetrically.
Add together the bond enthalpies for the reactants and record this number.
Enthalpies for steam and water are available from standard steam tables.
The alcohols have both higher entropies and enthalpies of activation than the ketones.
High melting enthalpies occur only with very high melting temperatures.
The Table hereafter summarizes the formation enthalpies of the studied carbides.
Specific enthalpies have been assigned to each interaction site in the first solvation shell.
The following results were obtained for the enthalpies of fusion,.
Melting temperatures and enthalpies of fusión were measured according to standard techniques.
Have been carried out so far, the free enthalpies of.
The apparent activation enthalpies for the elongation reaction have also been determined.
Historically, the vast majority of tabulated bond energy values are bond enthalpies.
The molar enthalpies of solution were correlated with the solvatochromic parameter of the solvents.
In these, the adsorption and evaporation enthalpies are utilized to generate heat or to cool.
Enthalpies of formation modeled at finite temperatures are in excellent agreement with available experimental results.
The sign, intensity, and trends of excess enthalpies and mutual solubilities are discussed.
The enthalpies of activation and of reaction are well correlated by the Marcus relation.
Generally, they can be considered completely amorphous, having non detectable melting enthalpies.
The melting points and enthalpies of fusión were measured during the second heating phase.
All these halides are colourless, high melting crystalline solids having high negative enthalpies of formation.
The vaporization enthalpies of DBN and DBU were derived from the vapor pressure correlations.
They contribute to the conformational and the net enthalpies of local and non-local interactions.
The enthalpies of metal-oxygen bonds were also estimated.
Table 3 also provides the corresponding enthalpies of fusión calculated from the raw materials values.
The enthalpies of formation were determined by “transposed temperature drop solution calorimetry” method.
The values between brackets are the transition enthalpies expressed in Kcal / mole.
The equation for enthalpies of reactions can then be expressed as,.
Apply Hess 's law to calculate standard enthalpy of reaction from standard enthalpies of formation.
The enthalpies which are involved are the same as previously, but with opposite signs.
