H2SO4 (aq) + 2 NaOH (aq) → 2 H2O (ℓ) + Na2SO4 (aq)

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Stoichiometry

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 H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L NaOH           Mass: g or Solution Volume: mL of Concentration: mol/L H2O            Mass: g Na2SO4         Mass: g Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(H2O (ℓ)) + 1ΔHf(Na2SO4 (aq))] - [1ΔHf(H2SO4 (aq)) + 2ΔHf(NaOH (aq))]
[2(-285.83) + 1(-1389.47)] - [1(-909.27) + 2(-470.09)] = -111.68 kJ
-111.68 kJ     (exothermic)

Entropy Change

[2ΔSf(H2O (ℓ)) + 1ΔSf(Na2SO4 (aq))] - [1ΔSf(H2SO4 (aq)) + 2ΔSf(NaOH (aq))]
[2(69.91) + 1(138.08)] - [1(20.08) + 2(48.25)] = 161.32 J/K
161.32 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(H2O (ℓ)) + 1ΔGf(Na2SO4 (aq))] - [1ΔGf(H2SO4 (aq)) + 2ΔGf(NaOH (aq))]
[2(-237.18) + 1(-1268.43)] - [1(-744.63) + 2(-419.18)] = -159.8 kJ
-159.80 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-159.78 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

9.9381727897e+027
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 125.