MgCO3 (s) + 1 H2SO4 (aq) → MgSO4 (aq) + H2O (ℓ) + 1 CO2 (g)

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Reaction Type:

Double Displacement/Decomposition of a Carbonate

Stoichiometry

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MgCO3          Mass: g
H2SO4          Mass: g  or Solution Volume: mL of Concentration: mol/L
MgSO4          Mass: g
H2O            Mass: g
CO2            Mass: g  or Gas Volume: L
Heat Released: kJ

Enthalpy of Reaction

[1ΔHf(MgSO4 (aq)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(CO2 (g))] - [1ΔHf(MgCO3 (s)) + 1ΔHf(H2SO4 (aq))]
[1(-1376.12) + 1(-285.83) + 1(-393.51)] - [1(-1095.79) + 1(-909.27)] = -50.4000000000001 kJ
-50.40 kJ     (exothermic)

Entropy Change

[1ΔSf(MgSO4 (aq)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(CO2 (g))] - [1ΔSf(MgCO3 (s)) + 1ΔSf(H2SO4 (aq))]
[1(-117.99) + 1(69.91) + 1(213.68)] - [1(65.69) + 1(20.08)] = 79.83 J/K
79.83 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(MgSO4 (aq)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(CO2 (g))] - [1ΔGf(MgCO3 (s)) + 1ΔGf(H2SO4 (aq))]
[1(-1199.43) + 1(-237.18) + 1(-394.38)] - [1(-1012.11) + 1(-744.63)] = -74.2500000000002 kJ
-74.25 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-74.20 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.0203778418e+013
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 98.

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