The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant.

A(g) + B(g) ? AB(g) Kc = 0.24

AB(g) + A(g) ? A2B(g) Kc = 3.8

2 A(g) + B(g) ? A2B(g) Kc = ?

A. 4.0

B. 0.91

C. 3.6

D. 16

E. 0.63

B. 091

Explanation:

When we add these two equilbria, the equilibrium constant for the resultant equilibrium is the product of the first two.

Notice that when we add the first two reactions in this question, we obtain the equilibrium for which we are seeking its equilibrium constant. Therefore,

A(g) + B(g) ? AB(g)           Kc₁ = [AB] / [A][B]          

                             +

AB(g) + A(g) ? A2B(g)       Kc₂ = [A₂B] /[ AB][A]

   2 A(g) + B(g)  ⇄ A₂B(g)    Kc₃ = [A₂B] / [A]²[B]

Kc₁Kc₂ =  [AB] / [A][B]  x  [A₂B] / [AB][A] =  [A₂B] / [A]²[B]

Thus,

Kc₃ = 0.24 x 3.8 = 0.91

This procedure is not limited to two reaction, it could done for more than two, as long as the desired equilibrium is the desired one.

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.