The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of and a

Chapter 20, Problem 14.122

(choose chapter or problem)

The gas-phase reaction of NO with \(\mathrm{F}_{2}\) to form NOF and F has an activation energy of \(E_{a}=6.3 \mathrm{kJ} / \mathrm{mol}\) and a frequency factor of \(A=6.0 \times 10^{8} M^{-1} \mathrm{s}^{-1}\). The reaction is believed to be bimolecular:

\(\mathrm{NO}(g)+\mathrm{F}_{2}(g) \longrightarrow \mathrm{NOF}(g)+\mathrm{F}(g)\)

(a) Calculate the rate constant at \(100^{\circ} \mathrm{C}\). (b) Draw the Lewis structures for the NO and the NOF molecules, given that the chemical formula for NOF is misleading because the nitrogen atom is actually the central atom in the molecule. (c) Predict the shape for the NOF molecule. (d) Draw a possible transition state for the formation of NOF, using dashed lines to indicate the weak bonds that are beginning to form. (e) Suggest a reason for the low activation energy for the reaction.