The equilibrium constant for the reaction, 12(s) + Br2 (g) 2 IB r (g) is 0.164 at 25°C.
(a) Calculate ∆rG° for this reaction.
(b) Bromine gas is introduced into a container with excess solid iodine.
The pressure and temperature are held at 0.164 atm and 25°C, respectively.
Find the partial pressure of IBr(g) at equilibrium. Assume that all the bromine is in the liquid form and that the vapour pressure of iodine is negligible.
(c) In fact, solid iodine has a measurable vapour pressure at 25°C. In this case, how would the calculation have to be modified?