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

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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  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.

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