# Question #7782e

##### 1 Answer

The molar enthalpy of solidification of pure sulfur is -4.123 kJ/mol.

#### Explanation:

If you want to get the correct sign for the molar entropy of solidification, you must use the formulas

**heat lost by sulfur = -heat gained by the calorimeter**

and

**moles × molar heat = -mass × specific heat capacity × change in temperature**

In symbols, these become

Here are the numbers we have to insert into the formulas.

Since your numbers are all given to 4 significant figures, we must use the mass of water to 4 significant figures.

The density of water at 32.40 °C is 0.9943 g/mL.

Hence,

The specific heat capacity of water is

This gives us

∴ The molar enthalpy of solidification of sulfur is -4.123 kJ/mol.

The negative sign tells us that the sulfur loses heat energy when it solidifies.

**NOTE**: There is either an error in your data or in my calculations, because the molar entropy of solidification of sulfur is -1.727 kJ/mol.