Final answer:
The boiling point of anhydrous magnesium sulfate (MgSO4) is not commonly reported because it decomposes before reaching its boiling point, typically resulting in the formation of magnesium oxide, sulfur dioxide, and oxygen.
Step-by-step explanation:
The boiling point of anhydrous magnesium sulfate (MgSO4) is not provided in standard reference materials because it decomposes before boiling. Typically, magnesium sulfate will lose its water of crystallization before reaching its boiling point, which can lead to decomposition into magnesium oxide (MgO), sulfur dioxide (SO2), and oxygen (O2).
For many salts, boiling points are not commonly reported because they tend to decompose at high temperatures before actually boiling. In practical settings, magnesium sulfate is used either in its hydrated form or in aqueous solution, so its boiling point as a pure compound is not often of concern.
The boiling point of anhydrous magnesium sulfate, MgSO4, can be determined by examining the colligative properties of solutions. Anhydrous magnesium sulfate does not contain any water molecules, so it does not exhibit boiling point elevation. Therefore, the boiling point of anhydrous magnesium sulfate is the same as that of the solvent, which in this case is water. The boiling point of water is 100 degrees Celsius (212 degrees Fahrenheit) at normal atmospheric pressure.