a) Acetone, C3H₂O, has a normal boiling point of 56.2 °C and the molar enthalpy of vaporization (AHm.vap) of 30.3 kJ/mol. Calculate AS vap (in J/K) for the vaporization of 0.758 mol of acetone. b) Find the molar entropy of vaporization (in J/(K-mol)) for a certain substance given that to vaporize 0.231 mol of that substance at -46.4 °C AH = 4.27 kJ.
a) Acetone, C3H₂O, has a normal boiling point of 56.2 °C and the molar enthalpy of vaporization (AHm.vap) of 30.3 kJ/mol. Calculate AS vap (in J/K) for the vaporization of 0.758 mol of acetone. b) Find the molar entropy of vaporization (in J/(K-mol)) for a certain substance given that to vaporize 0.231 mol of that substance at -46.4 °C AH = 4.27 kJ.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
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Problem 93QRT: The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar...
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Transcribed Image Text:a)
Acetone, C3H6O, has a normal boiling point of 56.2 °C and the molar enthalpy of vaporization
(AHm,vap) of 30.3 kJ/mol. Calculate ASvap (in J/K) for the vaporization of 0.758 mol of acetone.
b)
Find the molar entropy of vaporization (in J/(K-mol)) for a certain substance given that to vaporize
0.231 mol of that substance at -46.4 °C AH = 4.27 kJ.
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VIEWStep 2: Calculation of temperature in kelvin.
VIEWStep 3: Calculation of dSvap.
VIEWStep 4: Determine the given values.
VIEWStep 5: Calculation of molar enthalpy of vaporization.
VIEWStep 6: Calculation of temperature in Kelvin.
VIEWStep 7: Calculation of dSm,vap.
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