## 2 AgNO3 (aq) + 1 H2SO4 (aq) → Ag2SO4 (s) + 2 HNO3 (aq)

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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.

 AgNO3          Mass: g or Solution Volume: mL of Concentration: mol/L H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L Ag2SO4         Mass: g HNO3           Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Ag2SO4 (s)) + 2ΔHf(HNO3 (aq))] - [2ΔHf(AgNO3 (aq)) + 1ΔHf(H2SO4 (aq))]
[1(-715.88) + 2(-207.36)] - [2(-101.78) + 1(-909.27)] = -17.77 kJ
-17.77 kJ     (exothermic)

## Entropy Change

[1ΔSf(Ag2SO4 (s)) + 2ΔSf(HNO3 (aq))] - [2ΔSf(AgNO3 (aq)) + 1ΔSf(H2SO4 (aq))]
[1(200.41) + 2(146.44)] - [2(219.12) + 1(20.08)] = 34.97 J/K
34.97 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ag2SO4 (s)) + 2ΔGf(HNO3 (aq))] - [2ΔGf(AgNO3 (aq)) + 1ΔGf(H2SO4 (aq))]
[1(-618.48) + 2(-111.34)] - [2(-34.22) + 1(-744.63)] = -28.0900000000001 kJ
-28.09 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-28.20 kJ     (spontaneous) ## Equilibrium Constant, K (at 298.15 K)

83450.494817
This process is favorable at 25°C.

## Reference(s):

Zumdahl, Steven and Zumdahl, Susan A. Chemistry 9th ed.; Brooks/Cole: Belmont, CA, 2014; p 131.