H2SO4 (aq) + 2 NaHCO3 (s) → Na2SO4 (aq) + 2 H2O (ℓ) + 2 CO2 (g)

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Reaction Type:

Double Displacement/Decomposition of a Carbonate

Stoichiometry

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Heat Added: kJ
H2SO4          Mass: g  or Solution Volume: mL of Concentration: mol/L
NaHCO3         Mass: g
Na2SO4         Mass: g
H2O            Mass: g
CO2            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(Na2SO4 (aq)) + 2ΔHf(H2O (ℓ)) + 2ΔHf(CO2 (g))] - [1ΔHf(H2SO4 (aq)) + 2ΔHf(NaHCO3 (s))]
[1(-1389.47) + 2(-285.83) + 2(-393.51)] - [1(-909.27) + 2(-947.68)] = 56.48 kJ
56.48 kJ     (endothermic)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2SO4 (aq)) + 2ΔGf(H2O (ℓ)) + 2ΔGf(CO2 (g))] - [1ΔGf(H2SO4 (aq)) + 2ΔGf(NaHCO3 (s))]
[1(-1268.43) + 2(-237.18) + 2(-394.38)] - [1(-744.63) + 2(-851.86)] = -83.2000000000003 kJ
-83.20 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-86.93 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

3.7741610477e+014
This process is favorable at 25°C.