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?
Question
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?
Solution
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 process (in this case, it's the heat of fusion), and
- T is the absolute temperature (in Kelvin).
The heat of fusion (q) is given as 18.53 J/mol.
The temperature (T) during the fusion of ice is the freezing point of water, which is 0°C or 273.15 K.
Substituting these values into the formula, we get:
ΔS = 18.53 J/mol / 273.15 K = 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).
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