Standard Entropy for Liquid at Melting Point

[DiffusConfuse]

Homework Statement

The vapour pressures of a liquid have been measured and fit to the following equation:
Log₁₀ (mmHg) = -3571/T + 6.124
The melting point has been determined to be 392.7 K.
Calculate the standard entropy of the liquid at the melting point.

Homework Equations

The Attempt at a Solution

 

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Where's your attempt?

 

[DiffusConfuse]

My attempt was as follows:
T₁= 392.7 K P₁ = 0.8045 mmHg (from the equation, giving the vapour pressure of the LIQUID at the melting point).
T₂= 298.15 K P₂= 1.052E-3 mmHg

From the Clausius Clapeyron:

ln(0.8045/1.052E-3)= ΔH/R*(1/298.15 K - 1/392.7 K)

ΔH/R = 8221.89
ΔH = 68361 J/mol

ΔH/T = ΔS = 68361/392.7 = 174.07 J/mol K

However the answer is about twice this value and a Cp value given for the liquid is 250 J/mol K and the entropy of vaporisation is 117 J/mol K (2 additonal variables)