Chemical Equilibrium: The ICE table

Chemical Equilibrium: The ICE table

Presenter

Dr. Luis Bello

[e-mail]

https://www.linkedin.com/in/luisbello/

Previously we talked about

Learning Objectives

Identify the changes in concentration that occur for chemical species in equilibrium systems using the ICE table

Calculate equilibrium concentrations and equilibrium constants, using various algebraic approaches using the ICE table.

ICE

"I" stands for the initial concentrations (or pressures) for each species in the reaction mixture.

"C" represents the change in the concentrations (or pressures) for each species as the system moves towards equilibrium.

"E" represents the equilibrium concentrations (or pressures) of each species when the system is in a state of equilibrium.

EXAMPLE

Under certain conditions, the equilibrium constant Kc for the decomposition of PCl₅(g) into PCl₃(g) and Cl₂(g) is 0.0211.

What are the equilibrium concentrations of PCl₅, PCl₃, and Cl₂ in a mixture that initially contained only PCl5 at a concentration of 1.00 M?

Solution

Step 1

Determine the direction the reaction proceeds.

The balanced equation for the decomposition of PCl₅ is

PCl₅(g)⇌PCl₃(g)+Cl₂(g)

Step 2 Develop an ICE table.

Step 3. Solve for the change and the equilibrium concentrations.

Sources

Chemistry 2e. an OpenStax

https://openstax.org/books/chemistry-2e/pages/preface