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Consider the equilibrium of nitrogen dioxide and nitric oxide shown in the following reaction: ??2(?) ⇌ ??(?) + 1/2 ?2(?) Initially exactly one mole of nitrogen dioxide is placed in a vessel. At equilibrium, the volume of the vessel is adjusted so that the total pressure is exactly 1 bar. The gas is analyzed and the ratio of the following partial pressures was P NO / P NO2 =0.872 at a temperature of 426.85K. a) Determine the value of Kp at this set of conditions. b) Determine the standard free energy of this reaction under these conditions assuming that the gases are ideal. c) Using tabulated thermodynamic data (and assuming that the enthalpy and entropy are temperature independent) determine if this reaction is spontaneous at all temperatures. d) What set of non-standard conditions of system composition (if any) result in a change in the spontaneity of the reaction.

- November 14, 2022 - Edwin Tunner

Consider the equilibrium of nitrogen dioxide and nitric oxide shown in the following reaction:

??2(?) ⇌ ??(?) + 1/2 ?2(?)

Initially exactly one mole of nitrogen dioxide is placed in a vessel. At equilibrium, the volume of the vessel is adjusted so that the total pressure is exactly 1 bar.

The gas is analyzed and the ratio of the following partial pressures was P NO / P NO2 =0.872 at a temperature of 426.85K.

a) Determine the value of Kp at this set of conditions.

b) Determine the standard free energy of this reaction under these conditions assuming that the gases are ideal.

c) Using tabulated thermodynamic data (and assuming that the enthalpy and entropy are temperature independent) determine if this reaction is spontaneous at all temperatures.

d) What set of non-standard conditions of system composition (if any) result in a change in the spontaneity of the reaction.

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