[BROe]

I'm currently planning to run my first esterification reaction, Citric acid to Trimethyl citrate using methanol and 35%H₂SO₄ as a catalyst. Though I know I don't really need it, I wanted to see if I could find the equilibrium constant for the reaction as a sort of mental exercise.

The equation I'm using is one I dug up from my old Chemistry data booklet K_e = e^{(ΔH - TΔS)/(-RT)}
Where K is the equilibrium constant, H is the enthalpy of reaction in KJ/mol, S is the entropy of reaction in KJ/mol, T is temp. in Kelvin, and R is the gas constant 8.31.

I was able to find all the values I needed pretty easily as most of them were either available online or could be easily calculated. However, I have yet to find a value for the standard molar entropy for trimethyl citrate. I haven't found its value on any online tables I've looked at nor have I been able to find a way to calculate it using the data I have access to. If there are any pointers or sources anybody would like to share I would appreciate it.