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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Asked Oct 31, 2019
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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 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)
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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 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)

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Expert Answer

Step 1

Enthalpy of fusion for 1 mole of Al is 10699.45 J/mol

Initial temperature = 25 degC = 298.15K K

Final temperature = 750 degC = 1023.15K

Melting point = 660.46 deg C = 933.61K

The total entropy change is as follows,

...

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