The equation for the corrosion of iron to form iron (III) oxide (aka, rust) is: 4 Fe(s) + 3 O2(g) -à 2 Fe2O3(s) Using the following data, find the Gibbs free energy, ∆G for this process at 25° sC COMPOUND ∆Hf(Kj/mole) S° (J/K mole) Fe2O3 –826 90 Fe(s) 0 27 O2(g) 0 205
The equation for the corrosion of iron to form iron (III) oxide (aka, rust) is: 4 Fe(s) + 3 O2(g) -à 2 Fe2O3(s) Using the following data, find the Gibbs free energy, ∆G for this process at 25° sC COMPOUND ∆Hf(Kj/mole) S° (J/K mole) Fe2O3 –826 90 Fe(s) 0 27 O2(g) 0 205
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 82AE: Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the...
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- The equation for the corrosion of iron to form iron (III) oxide (aka, rust) is: 4 Fe(s) + 3 O2(g) -à 2 Fe2O3(s)
Using the following data, find the Gibbs free energy, ∆G for this process at 25° sC
|
COMPOUND |
∆Hf(Kj/mole) |
S° (J/K mole) |
|
Fe2O3 |
–826 |
90 |
|
Fe(s) |
0 |
27 |
|
O2(g) |
0 |
205 |
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