# Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from aninitial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquidaluminum at one bar pressure are 29.2 J mol1 K1 and 31.75 J mol1 K1, respectively. The specific enthalpyof fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is 26.98 gmol1.(Please explain as much as possible. Why did you use the equation? Or what conditions did you see from thequestion? etc)

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Do not copy from others, please! help_outlineImage TranscriptioncloseCalculate 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 mol1 K1 and 31.75 J mol1 K1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. 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) fullscreen
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Step 1

The entropy change for melting of aluminum can be calculated as help_outlineImage TranscriptioncloseGiven, Melting point of Al-660.46 C 660.46+273.15K=933.61K Enthalpy of fusion of Al = 3 96.57 Jg 10699.45 J mol Entropy change of melting: AH(fusion)xnumber of moles AS T (fusion) (10699.45Jmol2)(1mol) 933.61K -11.46JK fullscreen
Step 2

The entropy change for temperature of... help_outlineImage TranscriptioncloseEntropy change of change in temperature: T 660.46+273 .15K=933.61K T, 750+273.15K=1023 .1 5K Т, AS, =Cln т, (1023 .15 (31.75Jmol K)(1mol) In 933.61 2.90JK fullscreen

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