Answer :
Final answer:
The change in entropy, ∆S, for the phase change of 1.63 moles of methanol from solid to liquid at -97.6°C is 18.05 J/K·mol.
Explanation:
To determine ∆S, or the change in entropy, for the phase change of 1.63 moles of methanol from solid to liquid at -97.6°C, we can use the formula ∆S = ∆H/T, where ∆H is the change in enthalpy (or heat of fusion) and T is the absolute temperature in Kelvin. First, convert the temperature from Celsius to Kelvin by adding 273.15 to -97.6°C, which equals 175.55 K. Then, plug the values into the equation: ∆S = 3.17 kJ/mol / 175.55 K. Don't forget to convert ∆H from kJ to J, because the standard unit for entropy is J/K·mol. Therefore, ∆S = (3.17 kJ/mol * 1000 J/kJ) / 175.55 K = 18.05 J/K·mol.
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