# Calculating Entropy from Gibbs Free Energy?

I guess Cp = dH/dT= dq/dT=dS Thus SdT = integral of CpdT. From that ∆H is given and we can calculate ∆G. However, entropy for this reaction should be -7.4J/molK and I am getting like 26J/molK.

Also S is not ∆S which is a big flag in this working.

Entropy change is

$$\Delta S = \int \frac{\delta q}{T}$$

For a phase transformation this becomes

$$\Delta_{pt} S = \frac{\Delta_{pt} H}{T_{pt}}$$

Enthalpy and entropy depend on temperature as

$$\Delta H(T_2) - \Delta H(T_1) = \int C_p dT$$

$$\Delta S(T_2) - \Delta S(T_1) = \int \frac{C_p}{T} dT$$

The Gibbs energy change is

$$\Delta G = \Delta H - T \Delta S$$

The Gibbs energy change of the phase transformation at the transformation conditions is calculated directly from the enthalpy change and transition temperature.

To calculate the value at a different temperature, you must first calculate the enthalpy and entropy changes at the different temperature.