## 2 NaNO3 (s) + 1 H2SO4 (ℓ) → Na2SO4 (s) + 2 HNO3 (ℓ)

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## Reaction Type:

Double Displacement

## Stoichiometry

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 Heat Added: kJ NaNO3          Mass: g H2SO4          Mass: g Na2SO4         Mass: g HNO3           Mass: g

## Enthalpy of Reaction

[1ΔHf(Na2SO4 (s)) + 2ΔHf(HNO3 (ℓ))] - [2ΔHf(NaNO3 (s)) + 1ΔHf(H2SO4 (ℓ))]
[1(-1384.49) + 2(-173.22)] - [2(-466.68) + 1(-814)] = 16.4300000000001 kJ
16.43 kJ     (endothermic)

## Entropy Change

[1ΔSf(Na2SO4 (s)) + 2ΔSf(HNO3 (ℓ))] - [2ΔSf(NaNO3 (s)) + 1ΔSf(H2SO4 (ℓ))]
[1(149.49) + 2(155.6)] - [2(116.32) + 1(156.9)] = 71.15 J/K
71.15 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2SO4 (s)) + 2ΔGf(HNO3 (ℓ))] - [2ΔGf(NaNO3 (s)) + 1ΔGf(H2SO4 (ℓ))]
[1(-1266.83) + 2(-79.91)] - [2(-365.89) + 1(-690.07)] = -4.79999999999995 kJ
-4.80 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-4.78 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

6.93378561
This process is close to or at equilibrium 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 166.