Question

For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. Part B If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Cl2? Express your answer to two significant figures and include the appropriate units. Part C If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of BrCl? Express your answer to two significant figures and include the appropriate units.

Answer 1

Moles of Br,-025 mo Moles of Q2 3OL oles of Br2 0.083 M 3.0 L 055 mol 0.183M The given reaction is shown below Br2 + Cl2 22 BrCl 0.083 0.183 I: +2x E: (0,083-x) (0.183-x) +2x K - BrCijf Br2ICl2] (2x)2 7.0- (0,083-x)x(0.183-x) x-0.064 Equilibrium concentration of Bra (0.083-x) -(0.083-0.064) 0.019 M Equilibrium concentration of C12 (0183-x) -(0.183-0.064) -0, 12 м Equilibrium concentrati on of BrCl -2x - 2x0.064 -0.13M