Equilibrium Constant (Kc) Calculation and Explanation

What is the equilibrium constant (Kc)?

The equilibrium constant (Kc) is the rate of the reaction respective to the concentration of the reactants and the products formed.

The chemical reaction can be shown as: H2 + I2 ⇌ 2HI

Given,

The equilibrium constant (Kc) = 50.2

Initial moles of H2 = 1.39 moles

At equilibrium, the moles of hydrogen gas = 1.39 - x

Initial moles of I2 = 1.39 moles

At equilibrium, the moles of iodine = 1.39 - x

At equilibrium, the moles of hydrogen iodide = 2x

The equilibrium constant for the chemical reaction can be shown as: Kc = [HI]2 / [I2][H2]

We know that,

[HI]eq = 2x / 5

[H2]eq = (1.39-x) / 5

[I2]eq = (1.39-x) / 5

Substituting values in the above equation we get:

x = 1.084

Therefore, the equilibrium moles of hydrogen iodide is 2.168 moles.

The equilibrium moles of HI is 2.168 moles.

The equilibrium constant (Kc) is a crucial factor in understanding the balance of a chemical reaction. It represents the relationship between the concentrations of the reactants and the products at equilibrium. In this case, the equilibrium constant (Kc) for the reaction H2 + I2 ⇌ 2HI is 50.2.

To calculate the equilibrium moles of hydrogen iodide, we need to consider the initial moles of H2 and I2, as well as the equilibrium concentrations of all species involved. By applying the equilibrium constant expression and solving for the unknown variable x, we find that the equilibrium moles of HI is 2.168 moles.

This calculation showcases the dynamic nature of chemical reactions and the importance of equilibrium constants in quantifying reaction progress. Understanding these concepts is fundamental in chemistry and provides insights into reaction kinetics and thermodynamics.