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Enthalpy of Reaction
[1ΔHf(H2O2 (ℓ))] - [1ΔHf(H2 (g)) + 1ΔHf(O2 (g))]
[1(-187.78)] - [1(0) + 1(0)] = -187.78 kJ
-187.78 kJ (exothermic)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(H2O2 (ℓ))] - [1ΔGf(H2 (g)) + 1ΔGf(O2 (g))]
[1(-120.42)] - [1(0) + 1(0)] = -120.42 kJ
-120.42 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-120.40 kJ (spontaneous)
Equilibrium Constant, K (at 298.15 K)
This process is favorable at 25°C.
Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 223.