0.2mol of chlorine gas and 0.2mol of fluorine gas are placed in a sealed flask and heated to 2000K The following equilibrium occurred: (Cl2(g) + F2(g) = 2CIF (g) and at equilibrium the number of moles of CIF was equal to 0.267 mol, after that 0.1 mol was added of bromine and the following two equilibria occur 1- Cl2(g) + F2(g) = 2CIF(g) 2- Cl2(g) + Br2(g) = 2BrCl (g) At equilibrium, the number of moles of CIF was equal to 0.25 mol. Calculate the equilibrium constant for the second reaction

1Cl2(g)+F2(g)=2ClF(g)2Cl2(g)+Br2(g)=2BrCl(g) 4 0.25 CIF