## Mg (s) + 1 H2SO4 (aq) → MgSO4 (aq) + H2 (g)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Mg             Mass: g H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L MgSO4          Mass: g H2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(MgSO4 (aq)) + 1ΔHf(H2 (g))] - [1ΔHf(Mg (s)) + 1ΔHf(H2SO4 (aq))]
[1(-1376.12) + 1(0)] - [1(0) + 1(-909.27)] = -466.85 kJ
-466.85 kJ     (exothermic)

## Entropy Change

[1ΔSf(MgSO4 (aq)) + 1ΔSf(H2 (g))] - [1ΔSf(Mg (s)) + 1ΔSf(H2SO4 (aq))]
[1(-117.99) + 1(130.59)] - [1(32.69) + 1(20.08)] = -40.17 J/K
-40.17 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(MgSO4 (aq)) + 1ΔGf(H2 (g))] - [1ΔGf(Mg (s)) + 1ΔGf(H2SO4 (aq))]
[1(-1199.43) + 1(0)] - [1(0) + 1(-744.63)] = -454.8 kJ
-454.80 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-454.87 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

4.8077987725e+079
This process is favorable at 25°C.