What is the standard Gibbs free energy for this reaction? In kJ/mol At what temperature T_eq do the forward and reverse rusting reactions occur in equilibrium? In Kelvin?

Md Ariful Islam

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Md Ariful Islam

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$Delta"G"^@=Delta"H"^@-"T"Delta"S"^@$

Under standard conditions $"T" =298"K"$

$:.Delta"G"^@=-1648.4xx10^(3)-(298xx-543.7)$

$Delta"G"^@=-1486" ""kJ/mol"$

At equilibrium $Delta"G""=0$

$:.0=Delta"H"^@-"T"Delta"S"^@$

  • assuming the and changes don't change much with temperature we can use the standard values.

$:."T"=(Delta"H"^@)/(Delta"S"^@)$

$"T"=(-1648.4xx10^3)/(-543.7)" ""K"$

$"T"=3032" ""K"$

Strictly speaking, that is not the equation for rusting. This requires both air and water and the product, rust, is hydrated iron(III) oxide $sf(Fe_2O_3.xH_2O)$.

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