A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g) ↔ 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is .

 Thus the value of is 110.25

Explanation:

Initial moles of   = 0.500 mole

Initial moles of   = 0.500 mole

Volume of container = 1 L

Initial concentration of

Initial concentration of

equilibrium concentration of [/tex]

The given balanced equilibrium reaction is,

Initial conc.              0.500 M     0.500 M             0  M

At eqm. conc.    (0.500-x) M      (0.500-x) M     (2x) M

The expression for equilibrium constant for this reaction will be,

we are given : 2x = 0.84 M

x= 0.42

Now put all the given values in this expression, we get :

Thus the value of the equilibrium constant is 110.25

the answers would be

the first one and the second one