A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.536 mol of H2 present. At equilibrium, there are mol of Br2 present in the reaction vessel.

0.294 mol of present in the reaction vessel.

Explanation:

Initial moles of   = 0.682 mole

Initial moles of   = 0.440 mole

Volume of container = 2.00 L

Initial concentration of

Initial concentration of

equilibrium concentration of

The given balanced equilibrium reaction is,

Initial conc.              0.341 M     0.220 M         0  M

At eqm. conc.    (0.341-x) M      (0.220-x) M     (2x) M

The expression for equilibrium constant for this reaction will be,

we are given : (0.341-x) = 0.268 M

x= 0.073 M

Thus equilibrium concentration of = (0.220-x) M = (0.220-0.073) M = 0.147 M

Thus there are 0.294  mol of present in the reaction vessel.

explanation:

detials on each model with digrams