Reaction Type:
Double Displacement/Decomposition of Ammonium Hydroxide
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.
Enthalpy of Reaction
[1ΔHf(K3PO4 (aq)) + 3ΔHf(H2O (ℓ)) + 3ΔHf(NH3 (g))] - [1ΔHf((NH4)3PO4 (aq)) + 3ΔHf(KOH (s))]
[1(-2034.58) + 3(-285.83) + 3(-46.11)] - [1(-1674.91) + 3(-425.85)] = -77.9400000000001 kJ
-77.94 kJ (exothermic)
Entropy Change
[1ΔSf(K3PO4 (aq)) + 3ΔSf(H2O (ℓ)) + 3ΔSf(NH3 (g))] - [1ΔSf((NH4)3PO4 (aq)) + 3ΔSf(KOH (s))]
[1(85.75) + 3(69.91) + 3(192.34)] - [1(118.42) + 3(78.87)] = 517.47 J/K
517.47 J/K (increase in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(K3PO4 (aq)) + 3ΔGf(H2O (ℓ)) + 3ΔGf(NH3 (g))] - [1ΔGf((NH4)3PO4 (aq)) + 3ΔGf(KOH (s))]
[1(-1868.7) + 3(-237.18) + 3(-16.48)] - [1(-1256.91) + 3(-379.07)] = -235.56 kJ
-235.56 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-232.22 kJ (spontaneous)
Equilibrium Constant, K (at 298.15 K)
1.864759537e+041
This process is favorable at 25°C.