How much heat is liberated when 3.21g of iron (III) oxide are reduced by aluminum at constant pressure ( at 298.15 K)?
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The heat liberated will be 49.5 J
The reaction when iron (III) oxide is reduced by aluminum is given by :
2Al + Fe₂O₃ = Al₂O₃ + 2Fe
molecular weight of Fe₂O₃ is 160 gms
=> number of moles in 3.21 gms = 3.21/160 = 0.02
we know that heat liberated is given by,
ΔH = nRT
=> ΔH = 0.02 x 8.314 x 298.15
=> ΔH = 49.5 Joules
Hence the heat liberated when 3.21g of iron (III) oxide are reduced by aluminum will be 49.5 J
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