Question

At 25°C, the equilibrium constant K for the reaction in the solven 2BrCl = Br2 + Cl2 is 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine? 1.35 x 10-3M 2.70 x 10-3M 8.82 x 10-3 M 9.70 x 10-2 M. none of these choices is correct Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. D. NH4Is) + NH3(g) +HI(g) At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C. 0.103 atm 0.215 atm 0.232 atm 0.464 atm 2.00 atm The reaction system 32. POC13(g) = POCI(g) + Cl2(g) is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container? The forward reaction will proceed to establish equilibrium. The reverse reaction will proceed to establish equilibrium. The partial pressures of POCl; and POCI will remain steady while the partial pressure of chlorine increases. The partial pressure of chlorine remains steady while the partial pressures of POCl3 and POCl increase. The partial pressure of chlorine will increase while the partial pressure of POCI decreases. E.

Answer 1

The ICE table 2BrCI (g) Br(8)a (8) Initial (M) 0.0200 0 0.0300 Change (M) Equil (M) - 2x x x 0.0300 x 0.0200-2x BrC [BrCF (x)(0.0300+x) (0.0200-2x) Equilibrium constant, K 0.141 x 0.00135 Equilibrium concentration of Br Br (x) M =0.00135 M = 1.35x103 M