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

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## Reaction Type:

Double Displacement

## Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

 Heat Added: kJ NaNO3          Mass: g H2SO4          Mass: g Na2SO4         Mass: g HNO3           Mass: g or Gas Volume: L

## Enthalpy of Reaction

[1ΔHf(Na2SO4 (s)) + 2ΔHf(HNO3 (g))] - [2ΔHf(NaNO3 (s)) + 1ΔHf(H2SO4 (ℓ))]
[1(-1384.49) + 2(-135.06)] - [2(-466.68) + 1(-814)] = 92.75 kJ
92.75 kJ     (endothermic)

## Entropy Change

[1ΔSf(Na2SO4 (s)) + 2ΔSf(HNO3 (g))] - [2ΔSf(NaNO3 (s)) + 1ΔSf(H2SO4 (ℓ))]
[1(149.49) + 2(266.27)] - [2(116.32) + 1(156.9)] = 292.49 J/K
292.49 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2SO4 (s)) + 2ΔGf(HNO3 (g))] - [2ΔGf(NaNO3 (s)) + 1ΔGf(H2SO4 (ℓ))]
[1(-1266.83) + 2(-74.77)] - [2(-365.89) + 1(-690.07)] = 5.48000000000002 kJ
5.48 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.10962058516
This process is close to or at equilibrium at 25°C.

## Reference(s):

Kotz, John C. and Treichel, Paul. Chemistry & Chemical Reactivity 4th ed.; Thomson Brooks/Cole: Belmont, CA, 1999; p 173.