Question

How do you find the ${{K}_{eq}}$ of the equation?

Answer 1

The answer is based on the simple concept of the reactions in solutions part of the physical chemistry where Keq is nothing but the equilibrium constant of a reaction which is mainly for the reversible reaction. Cite an example for this so that required answer can be approached.

Complete answer:
In the lower classes of general chemistry, we have studied the very basic topic which is the reactions in solutions chapter which is included in the physical chemistry part. This concept deals with the study of the equilibrium constant, types of the reactions, thermodynamics and many other parameters.
We shall now understand the base of the equilibrium constant and how it can be calculated.
- Equilibrium constant which is denoted by ${{K}_{eq}}$ is defined as the value of its reaction quotient at chemical equilibrium which is a state approached by dynamic chemical system after sufficient time has elapsed at which there is no change in its concentration towards further change.
- The equilibrium constant of a reaction can be found by citing one example as shown below,
Let us calculate the equilibrium constant for the reaction where nitrogen reacts with chlorine to produce nitrogen trichloride with the data given as at equilibrium, the concentration of each gas were found to be $[{{N}_{2}}]=0.15M$,$[C{{l}_{2}}]=0.25M$ and $[NC{{l}_{3}}]=0.50M$
For this, let us write the reaction first,
${{N}_{2}}+3C{{l}_{2}}\to 2NC{{l}_{3}}$
Now, the equilibrium constant is nothing but the ratio of concentrations of product to that of the reactants and thus for the above example, we can write${{K}_{eq}}$ as,
${{K}_{eq}}=\dfrac{{{\left[ NC{{l}_{3}} \right]}^{2}}}{\left[ {{N}_{2}} \right]{{\left[ C{{l}_{2}} \right]}^{3}}}$
By substituting the values,
${{K}_{eq}}=\dfrac{{{\left[ 0.50 \right]}^{2}}}{\left[ 0.15 \right]{{\left[ 0.25 \right]}^{3}}}=106.7$
Thus, this example gives the required answer.

Note:
Note that the equilibrium constant value for the pure solids, pure liquids and solvents are having the value ‘1’ and it is dependent only on the concentrations of the solutes and thus the equilibrium constants are given for the solutes with particular concentrations.