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P3C.1 At 10K Cpm (Hg(s)) = 4.64 J K¯¹ mol¹. Between 10 K and the melting point of Hg(s), 234.3 K, heat capacity measurements indicate that the entropy increases by 57.74 J K ¹ mol ¹. The standard enthalpy of fusion of Hg(s) is 2322 Jmol-¹ at 234.3 K. Between the melting point and 298.0 K, heat capacity measurements indicate that the entropy increases by 6.85 J K¹ mol™¹. Determine the Third-Law standard molar entropy of Hg(1) at 298 K. P3C.2 The measurements described in Problem P3C.1 were extended to 343.9 K, the normal boiling point of Hg(1). Between the melting point and the boiling point, heat capacity measurements indicate that the entropy increases by 10.83 JK¯¹ mol¯¹. The standard enthalpy of vaporization of Hg(1) is 60.50 kJ mol¹ at 343.9 K. Determine the Third-Law standard molar entropy of Hg(g) at 343.9K (you will need some of the data from Problem P3C.1).

P3C.1 At 10K Cpm (Hg(s)) = 4.64 J K¯¹ mol¹. Between 10 K and the melting point of Hg(s), 234.3 K, heat capacity measurements indicate that the entropy increases by 57.74 J K ¹ mol ¹. The standard enthalpy of fusion of Hg(s) is 2322 Jmol-¹ at 234.3 K. Between the melting point and 298.0 K, heat capacity measurements indicate that the entropy increases by 6.85 J K¹ mol™¹. Determine the Third-Law standard molar entropy of Hg(1) at 298 K. P3C.2 The measurements described in Problem P3C.1 were extended to 343.9 K, the normal boiling point of Hg(1). Between the melting point and the boiling point, heat capacity measurements indicate that the entropy increases by 10.83 JK¯¹ mol¯¹. The standard enthalpy of vaporization of Hg(1) is 60.50 kJ mol¹ at 343.9 K. Determine the Third-Law standard molar entropy of Hg(g) at 343.9K (you will need some of the data from Problem P3C.1).

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
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P3C.1 At 10K Cpm (Hg(s)) = 4.64 J K¯¹ mol¹. Between 10 K and the melting point of Hg(s), 234.3 K, heat capacity measurements indicate that the entropy increases by 57.74 J K ¹ mol ¹. The standard enthalpy of fusion of Hg(s) is 2322 Jmol-¹ at 234.3 K. Between the melting point and 298.0 K, heat capacity measurements indicate that the entropy increases by 6.85 J K¹ mol™¹. Determine the Third-Law standard molar entropy of Hg(1) at 298 K. P3C.2 The measurements described in Problem P3C.1 were extended to 343.9 K, the normal boiling point of Hg(1). Between the melting point and the boiling point, heat capacity measurements indicate that the entropy increases by 10.83 JK¯¹ mol¯¹. The standard enthalpy of vaporization of Hg(1) is 60.50 kJ mol¹ at 343.9 K. Determine the Third-Law standard molar entropy of Hg(g) at 343.9K (you will need some of the data from Problem P3C.1).
Transcribed Image Text:P3C.1 At 10K Cpm (Hg(s)) = 4.64 J K¯¹ mol¹. Between 10 K and the melting point of Hg(s), 234.3 K, heat capacity measurements indicate that the entropy increases by 57.74 J K ¹ mol ¹. The standard enthalpy of fusion of Hg(s) is 2322 Jmol-¹ at 234.3 K. Between the melting point and 298.0 K, heat capacity measurements indicate that the entropy increases by 6.85 J K¹ mol™¹. Determine the Third-Law standard molar entropy of Hg(1) at 298 K. P3C.2 The measurements described in Problem P3C.1 were extended to 343.9 K, the normal boiling point of Hg(1). Between the melting point and the boiling point, heat capacity measurements indicate that the entropy increases by 10.83 JK¯¹ mol¯¹. The standard enthalpy of vaporization of Hg(1) is 60.50 kJ mol¹ at 343.9 K. Determine the Third-Law standard molar entropy of Hg(g) at 343.9K (you will need some of the data from Problem P3C.1).
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