## 2 Fe (s alpha) + 3 H2SO4 (aq) → Fe2(SO4)3 (aq) + 3 H2 (g)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Fe             Mass: g H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L Fe2(SO4)3      Mass: g H2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Fe2(SO4)3 (aq)) + 3ΔHf(H2 (g))] - [2ΔHf(Fe (s alpha)) + 3ΔHf(H2SO4 (aq))]
[1(-2824.87) + 3(0)] - [2(0) + 3(-909.27)] = -97.0599999999999 kJ
-97.06 kJ     (exothermic)

## Entropy Change

[1ΔSf(Fe2(SO4)3 (aq)) + 3ΔSf(H2 (g))] - [2ΔSf(Fe (s alpha)) + 3ΔSf(H2SO4 (aq))]
[1(-571.54) + 3(130.59)] - [2(27.28) + 3(20.08)] = -294.57 J/K
-294.57 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Fe2(SO4)3 (aq)) + 3ΔGf(H2 (g))] - [2ΔGf(Fe (s alpha)) + 3ΔGf(H2SO4 (aq))]
[1(-2243.09) + 3(0)] - [2(0) + 3(-744.63)] = -9.19999999999982 kJ
-9.20 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-9.23 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

40.912870495
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 140.