What is the entropy of CH3OH?
My CRC tables list 239.865 J/K*mol @ 298.15o K.
Do you also know the enthalpy?
deltaHof= -201.000 kJ/mol according to the CRC Handbook,1995-96 edition.
To determine the entropy of a substance, you can use the equation:
ΔS = ΔH / T
where ΔS is the change in entropy, ΔH is the change in enthalpy, and T is the temperature.
In this case, the given value -201.000 kJ/mol is the enthalpy change for the formation of CH3OH, denoted as ΔH°f. The temperature is given as 298.15 K.
To convert the enthalpy value from kJ/mol to J/mol, you multiply by 1000, as there are 1000 J in 1 kJ:
ΔH°f = -201.000 kJ/mol * 1000 J/kJ = -201000 J/mol
Now, substituting the values into the equation:
ΔS = (-201000 J/mol) / (298.15 K)
Calculating this equation will give you the value for the entropy of CH3OH.