How to Find the Equilibrium Constant

Science beakers
Getty Images/Yagi Studio
by Todd Helmenstine
Updated February 08, 2017

This example problem demonstrates how to find the equilibrium constant of a reaction from equilibrium concentrations of reactants and products.

Problem:

For the reaction

H2(g) + I2(g) ↔ 2 HI(g)

At equilibrium, the concentrations are found to be

[H2] = 0.106 M
[I2] = 0.035 M
[HI] = 1.29 M

What is the equilibrium constant of this reaction?

Solution

The equilibrium constant (K) for the chemical equation

aA + bB ↔ cC + dD

can be expressed by the concentrations of A,B,C and D at equilibrium by the equation

K = [C]c[D]d/[A]a[B]b

For this equation, there is no dD so it is left out of the equation.



K = [C]c/[A]a[B]b

Substitute for this reaction

K = [HI]2/[H2][I2]
K = (1.29 M)2/(0.106 M)(0.035 M)
K = 4.49 x 102

Answer:

The equilibrium constant of this reaction is 4.49 x 102.