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Abstract
Molar heat capacity of ammonium methanesulfonate NH4SO3CH3 was measured in the temperature range from 8.51 to 345.47 K by low-temperature vacuum adiabatic calorimetry. Heat capacity and the main thermodynamic functions (heat content, entropy and Gibbs energy) of NH4SO3CH3 in solid state were tabulated as a function of temperature from 10 K to 340 K. Enthalpy of NH4SO3CH3 dissolution in water was determined at 298.15 K by means of solution calorimetry. On the basis of the experimental data, the standard entropy, enthalpy and Gibbs energy of NH4SO3CH3 formation at 298.15 K were calculated. A second-order phase transition of NH4SO3CH3 was observed by adiabatic calorimetry at T = 272.6 ± 0.5 K.
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