For the reaction N2(g) + 2O2(g) → 2NO2(g) ΔH° = 66.4 kJ and ΔS° = -121.6 J/K The equilibrium constant for this reaction at 327.0 K is _______ . Assume that ΔH° and ΔS° are independent of temperature.
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Step 1
We know that ΔG° = ΔH° - TΔS°, where ΔG° is the standard Gibbs free energy change, ΔH° is the standard enthalpy change, T is the temperature in Kelvin, and ΔS° is the standard entropy change. Show more…
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