Question

Please do not copy the answer from others! Thank you!

Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol-1 k-and 31.75 J mol-1 k1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 Jg7. The molar mass of aluminum is 26.98 g mol1 (Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc)

Answer 1

Civen Moles of Imole AI 218.1S K Inital tem penatuxe 2s C fnal Tempenature So'c GSo +273. 15) k b23 -S K Heat Copacity 4 Solid Aluminium 29.2 Jmol'k 25t 1331s) k Heat Capauity liquid Aluminium 3.75 Jmolk Spea fic Enthalpy fusion Al AM396.57 Jg Meting point d fus AI660.46C-(23-1S+C60-46) k. 93361 k Process AL G A 0 7So C It is fo louing Skps into the divided AI U) AI O) Al s) AL G) 350'c 60.46C 2sc 660.46 C jmole Imole Imole IMol

AS nno moles AL S) AlS) Cp, mmolas Heat apacity 218.15 K 933.61 K mole Imole AS np ln T - Imole X 29 2 J molk In 933. K 298.15K Jkl 33-33 AS marsd Al AHFS AHRSpecific Enthalpy / Fosion 26 98 3 x 396 5 J9 933 61 K -11-y6 Jk AI U) A 0) 60.46C Imole Imol 933-6 K o23.1S K T

Imole X 31.7s Jkmol n 1023.15 K 933-61K - 2.91 Jk BStotal 2-91) Jk = (33. 33 + 11-46 aStotal