2 HNO3 (aq) + 1 Na2CO3 (aq) → 2 NaNO3 (aq) + H2O (ℓ) + 1 CO2 (g)

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Stoichiometry

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HNO3           Mass: g  or Solution Volume: mL of Concentration: mol/L
Na2CO3         Mass: g  or Solution Volume: mL of Concentration: mol/L
NaNO3          Mass: g
H2O            Mass: g
CO2            Mass: g  or Gas Volume: L
Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(NaNO3 (aq)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(CO2 (g))] - [2ΔHf(HNO3 (aq)) + 1ΔHf(Na2CO3 (aq))]
[2(-447.46) + 1(-285.83) + 1(-393.51)] - [2(-207.36) + 1(-1157.34)] = -2.20000000000005 kJ
-2.20 kJ     (exothermic)

Entropy Change

[2ΔSf(NaNO3 (aq)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(CO2 (g))] - [2ΔSf(HNO3 (aq)) + 1ΔSf(Na2CO3 (aq))]
[2(205.44) + 1(69.91) + 1(213.68)] - [2(146.44) + 1(61.1)] = 340.49 J/K
340.49 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(NaNO3 (aq)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(CO2 (g))] - [2ΔGf(HNO3 (aq)) + 1ΔGf(Na2CO3 (aq))]
[2(-373.24) + 1(-237.18) + 1(-394.38)] - [2(-111.34) + 1(-1051.7)] = -103.66 kJ
-103.66 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-103.72 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.4502964962e+018
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 137.

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