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.

according to kinetic-molecular theory, the following would not be considered an ideal gas:

a gas at very low volumes, when gas particles are very close together

a gas at very low temperatures, when gas particles have very little kinetic energy a gas

a gas with highly polar molecules that have very strong intermolecular forces

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3 1/4 %

explanation: