At a high temperature, equal concentrations of 0.160 mol/l of h2(g) and i2(g) are initially present in a flask. the h2 and i2 react according to the balanced equation below. h2(g) + i2(g) 2 hi(g)when equilibrium is reached, the concentration of h2(g) has decreased to 0.036 mol/l. what is the equilibrium constant, kc, for the reaction?

Explanation:

The given reaction is as follows.

Initial :                  0.160    0.160          0  

Change :                  -x           -x              2x

Equilibrium:        0.160 - x    0.160 - x       x

It is given that = [0.160 - x] = 0.036 M

and,                 = [0.160 - x] = 0.036 M      

so,                             x = (0.160 - 0.036) M

                                    = 0.124 M

As, [HI] = 2x.

So,           [HI] =

                       = 0.248 M

As it is known that expression for equilibrium constant is as follows.

                                  =

                                  = 47.46

Thus, we can conclude that the equilibrium constant, Kc, for the given reaction is 47.46.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).