Iodine and bromine react to give iodine monobromide, IBr. Ilg) + Br2(g) 2 Br(g) What is the equilibrium composition of a mixture at 145 C that initially contained 0.0019 mol each of iodine and bromine in a 5.0-L vessel? The equilibrium constant K, for this reaction at 145 C is 108.

Equilibrium concentration of = 0.00006 M

equilibrium concentration of = 0.00006 M

and equilibrium concentration of  = 0.00064 M

Explanation:

Initial moles of   = 0.0019 mole

Volume of container = 5.0 L

Initial concentration of  

initial concentration of

The chemical reaction for the decomposition of phosgene follows the equation:

Initial conc.        0.00038 M       0.00038 M       0

At eqm. conc.    ( 0.00038-x) M   (0.00038-x) M  (2x) M

The expression for equilibrium constant for this reaction will be,

Thus equilibrium concentration of  = (0.00038-x) M =(0.00038-0.00032) M = 0.00006 M

equilibrium concentration of = (0.00038-x) M =(0.00038-0.00032) M = 0.00006 M

equilibrium concentration of = 2x M = 2(0.00032) M=0.00064 M

i think its 100.

hope this !