Step 1:

The equilibrium constant K is 1.6 * 10^-5.

Initially 5.2 moles of NOCl is placed in 2.0 L of container.

Initial amount of NOCl is

The chemical equation is .

Let x be the concentration of .

Then concentration of NO at equilibrium be 2x.

Step 2:

Now complete the give ICE table.

Equilibrium Amount = Initial amount + Change in amount.

(i) Find the change in amount of NOCl.

From the table, Equilibrium amount of NOCl is 2.6-2x.

Initial amount of NOCl is 2.6 M.

Equilibrium Amount = Initial amount + Change in amount.

Change in amount of NOCl is -2x.

(ii) Find the change in amount of NO.

Initially the amount of NO is 0 M.

Equilibrium Amount of NO is 2x

Equilibrium Amount = Initial amount + Change in amount.

2x = 0 + Change in amount.

Change in amount of NOCl is 2x.

(iii) Find the change in amount of Cl₂.

Initially the amount of Cl₂ is 0 M.

Equilibrium Amount of Cl₂ is x

Equilibrium Amount = Initial amount + Change in amount.

x = 0 + Change in amount.

Change in amount of Cl₂ is x.

Step 3:

Initial Amount
Change in Amount
Equilibrium amount

Solution:

Initial Amount
Change in Amount
Equilibrium amount

Step 1:

The equilibrium constant K is 1.6 * 10^-5.

The concentrations of NOCl, NO and Cl₂ is 2.6-2x, 2x and x [From (a)].

Definition of equilibrium constant:

Equilibrium constant  is the ratio of the concentrations of products to the concentration of reactants.

.

The chemical reaction is .

Solutions of is x = -0.02977, 0.01489 and 0.01489.

Since concentration cannot be negative, x = 0.01489.

Concentration of [Cl₂] is

Concentration of [NO] is

Concentration of [NOCl] is 

Solution:

Concentration of [Cl₂] is

Concentration of [NO] is

Concentration of [NOCl] is