The standard entropy of Fe(s) at 298 K is 27.30 J K-¹ mol-¹. Assume that the heat capacity of Fe(s) is given by Cpm (Fe, s) J K ¹ mol-¹ = 23.97449 +8.36775 × 10-2 +2.77 × 10-5²2 The melting point is 1536 °C and the heat of fusion under these conditions is 12.4 kJ mol-¹. Assume that the heat capacity of Fe(/) is given by Cp,m (Fe, 1) = 46.024 - 1.884667 × 10-³ T JK mol K Calculate AH for the transformation Fe(s, 25 °C) →→→ Fe(1, 2,258 °C) Answer in kJ mol¹ to 1 decimal place (e.g. 176.2)
The standard entropy of Fe(s) at 298 K is 27.30 J K-¹ mol-¹. Assume that the heat capacity of Fe(s) is given by Cpm (Fe, s) J K ¹ mol-¹ = 23.97449 +8.36775 × 10-2 +2.77 × 10-5²2 The melting point is 1536 °C and the heat of fusion under these conditions is 12.4 kJ mol-¹. Assume that the heat capacity of Fe(/) is given by Cp,m (Fe, 1) = 46.024 - 1.884667 × 10-³ T JK mol K Calculate AH for the transformation Fe(s, 25 °C) →→→ Fe(1, 2,258 °C) Answer in kJ mol¹ to 1 decimal place (e.g. 176.2)
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
Section16.3: Measuring Dispersal Of Energy: Entropy
Problem 16.3CE
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