Textbook Problem

Equilibrium constants can be measured for the dissociation of Lewis acid-base complexes such as the dimethyl ether complex of BF₃, (CH₃)₂O→BF₃. The value of K (here K_p) for the reaction is 0.17 at 125 °C.

(CH₃)₂O→BF₃(g) ⇄ BF₃(g) + (CH₃)₂O(g)

1. (a) Describe each product as a Lewis acid or a Lewis base.
2. (b) If you place l.00 g of the complex in a 565-mL flask at 125°C, what is the total pressure in the flask when equilibrium is established? What are the equilibrium partial pressures of the Lewis acid, the Lewis base, and the complex?