enthalpy of fusion

It is also possible to predict solubility from other physical constants such as the enthalpy of fusion.

Enthalpy of fusion is the measure of the energy needed to change a substance from a solid to a liquid.

Differential scanning calorimetry gives information on melting point together with its enthalpy of fusion.

The enthalpy of fusion is almost always a positive quantity; helium is the only known exception.

Differential Scanning Calorimeter gives melting point and enthalpy of fusion.

Enthalpy of fusion or melting.

The refrigerant, usually non-toxic, can absorb a considerable amount of heat, since its enthalpy of fusion is high.

Water (ice) has an unusually high enthalpy of fusion and a convenient melting temperature (one accessible by household freezers).

In the specific cases of melting and freezing, it's called enthalpy of fusion or heat of fusion.

The integration constant K may be determined for a pure component with a melting temperature and an enthalpy of fusion Eq.

The dynamically disordered nature of the β-phase is partly responsible for the low enthalpy of fusion of silica.

The standard molar enthalpy of fusion is a measure of the energy needed to overcome the forces of attraction that exist between particles in the solid state.

Enthalpy of fusion, defined as the enthalpy change required to completely change the state of one mole of substance between solid and liquid states.

The enthalpy of sublimation (also called heat of sublimation) can be calculated as the enthalpy of fusion plus the enthalpy of vaporization.

The standard molar enthalpy of fusion, is the enthalpy change that accompanies the fusion of one mole of a substance at its melting point at one atmosphere pressure.

That amount of motional energy from the surroundings that is required for melting or boiling is called the phase change energy, specifically the enthalpy of fusion or of vaporization, respectively.

Moreover, its enthalpy of fusion is lower than the enthalpies of fusion of both n-pentane and isopentane, thus indicating that its high melting point is due to an entropy effect.

The enthalpy of fusion or heat of fusion is the change in enthalpy resulting from heating a given quantity of a substance to change its state from a solid to a liquid.

The heat δQ for this process is the energy required to change water from the solid state to the liquid state, and is called the enthalpy of fusion, i.e. ΔH for ice fusion.

The heat energy, or enthalpy, associated with a solid to liquid transition is the enthalpy of fusion and that associated with a solid to gas transition is the enthalpy of sublimation.

The energy released upon freezing is a latent heat, and is known as the enthalpy of fusion and is exactly the same as the energy required to melt the same amount of the solid.

Helium-3 has a negative enthalpy of fusion at temperatures below 0.3 K. Helium-4 also has a very slightly negative enthalpy of fusion below 0.8 K. This means that, at appropriate constant pressures, these substances freeze with the addition of heat.