## Na2SO4 (s) + 4 C (s graphite) → Na2S (s) + 4 CO (g)

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## Stoichiometry

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 Heat Added: kJ Na2SO4         Mass: g C              Mass: g Na2S           Mass: g CO             Mass: g or Gas Volume: L

## Enthalpy of Reaction

[1ΔHf(Na2S (s)) + 4ΔHf(CO (g))] - [1ΔHf(Na2SO4 (s)) + 4ΔHf(C (s graphite))]
[1(-373.21) + 4(-110.54)] - [1(-1384.49) + 4(0)] = 569.12 kJ
569.12 kJ     (endothermic)

## Entropy Change

[1ΔSf(Na2S (s)) + 4ΔSf(CO (g))] - [1ΔSf(Na2SO4 (s)) + 4ΔSf(C (s graphite))]
[1(97.91) + 4(197.9)] - [1(149.49) + 4(5.69)] = 717.26 J/K
717.26 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2S (s)) + 4ΔGf(CO (g))] - [1ΔGf(Na2SO4 (s)) + 4ΔGf(C (s graphite))]
[1(-359.82) + 4(-137.28)] - [1(-1266.83) + 4(0)] = 357.89 kJ
357.89 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

1.9810520094e-063
This process is not favorable at 25°C.

## Reference(s):

Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 167.