Na2SO4 (aq) + 1 BaCl2 (aq) → 2 NaCl (aq) + BaSO4 (s)

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Stoichiometry

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Na2SO4         Mass: g  or Solution Volume: mL of Concentration: mol/L
BaCl2          Mass: g  or Solution Volume: mL of Concentration: mol/L
NaCl           Mass: g
BaSO4          Mass: g
Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(NaCl (aq)) + 1ΔHf(BaSO4 (s))] - [1ΔHf(Na2SO4 (aq)) + 1ΔHf(BaCl2 (aq))]
[2(-407.25) + 1(-1473.19)] - [1(-1389.47) + 1(-871.9)] = -26.3200000000002 kJ
-26.32 kJ     (exothermic)

Entropy Change

[2ΔSf(NaCl (aq)) + 1ΔSf(BaSO4 (s))] - [1ΔSf(Na2SO4 (aq)) + 1ΔSf(BaCl2 (aq))]
[2(115.48) + 1(132.21)] - [1(138.08) + 1(122.56)] = 102.53 J/K
102.53 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(NaCl (aq)) + 1ΔGf(BaSO4 (s))] - [1ΔGf(Na2SO4 (aq)) + 1ΔGf(BaCl2 (aq))]
[2(-393.15) + 1(-1362.31)] - [1(-1268.43) + 1(-823.3)] = -56.8800000000001 kJ
-56.88 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-56.89 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

9236328067.6
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 139.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 159.

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