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I'd like to know the standard molar entropy S0solid for ammonium bicarbonate to use in an example in class, to calculate ΔS0 for the reaction, NH4HCO3(s) → NH3(g) + H2O(g) + CO2(g).

Already checked: Wikipedia, NIST Chemistry WebBook, Google. I don't have access to the CRC handbook.

(Arthur and Chester Miller already found the standard enthalpy of formation for ammonium bicarbonate, in this forum, in 2016; and it's in the German Wikipedia.)

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“Standard Thermodynamic Properties of Chemical Substances”, in CRC Handbook of Chemistry and Physics, 90th Edition (CD-ROM Version 2010), David R. Lide, ed., CRC Press/Taylor and Francis, Boca Raton, FL. gives values for the standard molar enthalpy of formation $\Delta_\mathrm fH^\circ$, the standard molar Gibbs energy of formation $\Delta_\mathrm fG^\circ$, and the standard molar entropy $S^\circ$ (all at $T=298.15\ \mathrm K$ and $p=100\ \mathrm{kPa}=1\ \mathrm{bar}$) of crystalline ammonium hydrogen carbonate as follows. $$\begin{align} \Delta_\mathrm fH^\circ&=-849.4\ \mathrm{kJ/mol}\\ \Delta_\mathrm fG^\circ&=-665.9\ \mathrm{kJ/mol}\\ S^\circ&=120.9\ \mathrm{J/(mol\ K)} \end{align}$$

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