Question

Suppose a 500. ml flask is filled with 1.3 mol of Br2, 2.0 mol of OC1, and 1.2 mol of BrCl. The following reaction becomes possible: Br2(g) + OC12(g) = BroCl (g) + BrCl (g) The equilibrium constant K for this reaction is 0.766 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. xs ?

Answer 1

Br. (9) + Ou2 (9) - Broce (9) + Initial Briel 1.2 mole moles disarociated & formed at equili- het a be the l-brium At equilibrium 1.3-1 (moles 2-x ot 1.2 ta

= & Equilibrium (K) constant Broce x Brex Bree Pace Now using Equation releal Gas PV = nRT P = nRT - Suice vol (V) R (Cas constants & Temp. (T)] are constant ole it gets already included in K. So, we write it as n (no. of moles) A K = Broce x вч, х Bell noq, 0.766 - 2 (1. (1.3-2) (2-1) 0.766 1.2x + x² 2.6-3.3x + x² 1.99 - 2.52x + 0.766x² = 1.20+ x² 10.234 x² +3.72x - 1.99 = 0