Question

Recall that when a reaction is at equilibrium, the forward and reverse reactions occur at the same rate. To illustrate this idea, consider the reaction of A (small, red spheres) and B (large, blue spheres) to form AB.

A+B ⇌ AB

Notice that the reaction never stops. Even after several minutes, there is A and B left unreacted, and the forward and reverse reactions continue to occur. Also note that amounts of each species (i.e., their concentrations) stay the same.

Required:
What is the value of the equilibrium constant for this reaction?
Assume each atom or molecule represents a 1 M concentration of that substance.

Answer 1

Equilibrium constant Kc = [x]² / [A - x] [B - x]

Step-by-step explanation:

The equilibrium constant is defined as the ratio of the concentration of the products to that of the reactants at equilibrium

ie Kc = [products] / [reactants].

The balanced equation of the reaction is given as : A + B ⇄ AB

At the beginning of the reaction,

Initial concentration I = A = 1M

B = 1M

AB = 0M

After a period of time and assuming 'x' to be the concentration of product AB formed, the concentrations become

C = reactant A = [A - x] M

rectant B = [B - x] M

Product AB = [x] [x] M

At equilibrium, the concentrations are,

E = rectant A = [A - x] M

reactant B = [B - x] M

product AB = [x]² M

therefore , the equilibrium constant, Kc = [products]/[reactants]

= [x]² / [A - x] [B - x]