Cl2 (g) + 2 NaOH (aq) → NaCl (aq) + NaClO (aq) + 1 H2O (ℓ)

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Stoichiometry

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Cl2            Mass: g  or Gas Volume: L
NaOH           Mass: g  or Solution Volume: mL of Concentration: mol/L
NaCl           Mass: g  or Solution Volume: mL of Concentration: mol/L
NaClO          Mass: g  or Solution Volume: mL of Concentration: mol/L
H2O            Mass: g

Enthalpy of Reaction

[1ΔHf(NaCl (aq)) + 1ΔHf(NaClO (aq)) + 1ΔHf(H2O (ℓ))] - [1ΔHf(Cl2 (g)) + 2ΔHf(NaOH (aq))]
[1(-407.25) + 1(-347.21) + 1(-285.83)] - [1(0) + 2(-470.09)] = -100.11 kJ
-100.11 kJ     (exothermic)

Entropy Change

[1ΔSf(NaCl (aq)) + 1ΔSf(NaClO (aq)) + 1ΔSf(H2O (ℓ))] - [1ΔSf(Cl2 (g)) + 2ΔSf(NaOH (aq))]
[1(115.48) + 1(100.84) + 1(69.91)] - [1(222.97) + 2(48.25)] = -33.24 J/K
-33.24 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(NaCl (aq)) + 1ΔGf(NaClO (aq)) + 1ΔGf(H2O (ℓ))] - [1ΔGf(Cl2 (g)) + 2ΔGf(NaOH (aq))]
[1(-393.15) + 1(-298.72) + 1(-237.18)] - [1(0) + 2(-419.18)] = -90.6900000000001 kJ
-90.69 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-90.20 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

7.7461280315062E+15
This process is favorable at 25°C.

Reference(s):

Atkins, Jones, and Laverman. Chemical Principles 6th ed.; W.H. Freeman and Company: New York, NY, 2013; p F94.

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