The normal heat of fusion of water is 18.53 J/mol. Calculate the change of entropy of the system that 1 mole of solid water is changed to liquid water?

To calculate the change in entropy (ΔS) when 1 mole of solid water changes to liquid water, we can use the formula:

ΔS = q/T

where:

• q is the heat absorbed or released during the phase change (in this case, the heat of fusion), and
• T is the absolute temperature (in Kelvin).

The heat of fusion (q) is given as 18.53 J/mol.

However, we don't have the temperature (T) given in the problem. The temperature at which water melts (i.e., changes from solid to liquid) is 0 degrees Celsius, which is equivalent to 273.15 Kelvin.

So, we can substitute these values into the formula:

ΔS = (18.53 J/mol) / (273.15 K)

This gives us:

ΔS = 0.0678 J/(mol*K)

So, the change in entropy when 1 mole of solid water changes to liquid water is 0.0678 J/(mol*K).