## 2 NaCl (aq) + 2 H2O (ℓ) → H2 (g) + Cl2 (g) + 2 NaOH (aq)

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## Stoichiometry

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 Heat Added: kJ NaCl           Mass: g or Solution Volume: mL of Concentration: mol/L H2O            Mass: g H2             Mass: g or Gas Volume: L Cl2            Mass: g or Gas Volume: L NaOH           Mass: g

## Enthalpy of Reaction

[1ΔHf(H2 (g)) + 1ΔHf(Cl2 (g)) + 2ΔHf(NaOH (aq))] - [2ΔHf(NaCl (aq)) + 2ΔHf(H2O (ℓ))]
[1(0) + 1(0) + 2(-470.09)] - [2(-407.25) + 2(-285.83)] = 445.98 kJ
445.98 kJ     (endothermic)

## Entropy Change

[1ΔSf(H2 (g)) + 1ΔSf(Cl2 (g)) + 2ΔSf(NaOH (aq))] - [2ΔSf(NaCl (aq)) + 2ΔSf(H2O (ℓ))]
[1(130.59) + 1(222.97) + 2(48.25)] - [2(115.48) + 2(69.91)] = 79.28 J/K
79.28 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(H2 (g)) + 1ΔGf(Cl2 (g)) + 2ΔGf(NaOH (aq))] - [2ΔGf(NaCl (aq)) + 2ΔGf(H2O (ℓ))]
[1(0) + 1(0) + 2(-419.18)] - [2(-393.15) + 2(-237.18)] = 422.3 kJ
422.30 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
422.34 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.0283103274e-074
This process is not favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 94.