Hydrogen peroxide (H₂O₂) decomposes according to the following equation. H₂O₂(l) → H₂O(l) + ½O₂(g) .
What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol, ΔS° = 70.1 J/K • mol, R = 8.314 J/K • mol)

Question

Quizplus · Accepted Answer

Using the equation:
ΔG° = ΔH° - TΔS°
We can calculate the standard Gibbs free energy change of the reaction:
ΔG° = (-98.2 kJ/mol) - (298 K)(70.1 J/K•mol/1000) = -121.6 kJ/mol

Then, using the equation:
ΔG° = -RTln(K)
We can solve for the equilibrium constant:
K = e^(-ΔG°/RT) = e^(-(-121.6 kJ/mol)/(8.314 J/K•mol)(298 K)) = 7.4 × 10^20

Therefore, the correct answer is D.

Hydrogen Peroxide (H2O2) Decomposes According to the Following Equation

Hydrogen Peroxide (H₂O₂) Decomposes According to the Following Equation