Molecular nitrogen has a strong triple bond and, thus, high temperatures are required to achieve any significant dissociation, as compared with less strongly bonded diatomic molecules. Explore the temperature dependence of the equilibrium reaction N₂ ⇔ N + N by calculating the equilibrium mole fractions of N and N₂ and the fraction of N₂ dissociated at 1 atm for temperatures of 1000, 2000, 3000, and 4000 K. Plot your results on a logarithmic scale. Also compare the dissociation fraction for 3000 K with the corresponding dissociation fraction for oxygen, which you can calculate from Example 13.1.

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Example 13.1 Dissociation of Oxygen At high temperatures, oxygen molecules dissociate to produce O atoms via the reaction 0₂0 +0. Determine the equilibrium partial pressures and mole fractions of O and O₂ at 1 atm and 3000 K. P, T fixed Xo = ? Xo₂ = ?