## Cu(NO3)2 (aq) + 2 KOH (aq) → Cu(OH)2 (s) + 2 KNO3 (aq)

Back to reactions list

## 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.

 Cu(NO3)2       Mass: g or Solution Volume: mL of Concentration: mol/L KOH            Mass: g or Solution Volume: mL of Concentration: mol/L Cu(OH)2        Mass: g KNO3           Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Cu(OH)2 (s)) + 2ΔHf(KNO3 (aq))] - [1ΔHf(Cu(NO3)2 (aq)) + 2ΔHf(KOH (aq))]
[1(-450.2) + 2(-459.76)] - [1(-349.95) + 2(-482.39)] = -54.99 kJ
-54.99 kJ     (exothermic)

## Entropy Change

[1ΔSf(Cu(OH)2 (s)) + 2ΔSf(KNO3 (aq))] - [1ΔSf(Cu(NO3)2 (aq)) + 2ΔSf(KOH (aq))]
[1(108.37) + 2(248.94)] - [1(193.3) + 2(91.75)] = 229.45 J/K
229.45 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cu(OH)2 (s)) + 2ΔGf(KNO3 (aq))] - [1ΔGf(Cu(NO3)2 (aq)) + 2ΔGf(KOH (aq))]
[1(-372.79) + 2(-394.64)] - [1(-157.16) + 2(-440.58)] = -123.75 kJ
-123.75 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-123.40 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

4.8002998356e+021
This process is favorable at 25°C.

## Reference(s):

Silberberg, Martin S. Chemistry: The Molecular Nature of Matter and Change 4th ed.; McGraw-Hill: Boston, MA, 2006; p 127.