Online Water Boiling Point Calculator

Triple point of water The single combination of pressure and temperature at which liquid water, solid ice, and water vapor can coexist in a stable equilibrium occurs at approximately 273.1575 K (0.0075 °C; 32.0135 °F) and a partial vapor pressure of 611.657 pascals (6.11657 mbar; 0.00603659 atm).

42.2

When comparing vapor pressures we need to be making comparisons at the same temperature. Thus at room temperature, the substance with the lowest boiling point will have the highest vapor pressure (easiest to get into the gas phase). The substance with the highest boiling point will have the lowest vapor pressure.

propanone

The chemical element with the lowest boiling point is Helium and the element with the highest boiling point is Tungsten.

Remember, the greater the concentration of particles, the lower the freezing point will be. 0.1mCaI2 will have the lowest freezing point, followed by 0.1mNaCl, and the highest of the three solutions will be 0.1mC6H12O6, but all three of them will have a lower freezing point than pure water.

Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions, but not upon the identity of the solute. Colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.

These colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.

Colligative Properties depend on how many solute particles are present as well as the solvent amount, but they do NOT depend on the type of solute particles, although do depend on the type of solvent. Anomalous colligative properties are colligative properties that deviate from the ideal colligative behavior.

… statement of this condition is Raoult’s law, which is valid for many highly dilute solutions and for a limited class of concentrated solutions, namely, those in which the interactions between the molecules of solute and solvent are the same as those between the molecules of each substance by itself.

Raoult’s law implies that the partial vapor pressure of a solvent in a solution (or mixture) is identical to or equal to the vapor pressure of a pure solvent multiplied by the mole fraction of the solution. …

The partial pressure is the pressure the gas if the gas were in the same volume and temperature by itself. Dalton’s law states the total pressure of a mixture of ideal gases is the sum of the partial pressure of each individual gas.

The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas: Ptotal=P1+P2+… +Pn. + P n . The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas.

The pressure exerted by an individual gas in a mixture is known as its partial pressure. Assuming we have a mixture of ideal gases, we can use the ideal gas law to solve problems involving gases in a mixture.