# LeChatelier's Principle: Disruption and Re-Establishment of Equilibrium Video

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Lesson Transcript
Instructor: Amy Meyers

Amy holds a Master of Science. She has taught science at the high school and college levels.

Learn how Le Chatelier's Principle describes the disruption and re-establishment of equilibrium. Learn to explain the factors that disrupt equilibrium, such as concentration, temperature, and pressure. Learn how each of these factors affects a system in equilibrium.

## Le Chatelier's Principle

Look at a closed soda bottle. What do you see? Without shaking it up, do you see any gas in there? Any bubbles? Any mist? You most likely don't see gas, mist, or many bubbles. That is because the pressure in the bottle keeps all the bubbles and gas in the solution. The liquid and gas are in equilibrium.

Now open the bottle. What do you see? You probably see bubbles, foam, or mist. Why? Because you have changed the amount of pressure on the liquid and the gas no longer stays in solution. The change in pressure caused the liquid and gas solution to no longer be in equilibrium. Eventually, as you know, most of the gas will leave the liquid and the soda will go flat. When this happens, the liquid and gas are back in equilibrium, just a different equilibrium than the closed bottle.

Equilibrium is explained in chemistry by Le Chatelier's Principle, which states that any change in a substance on one side of the equation in concentration, temperature, or pressure results in an equilibrium shift to oppose the change until a new equilibrium is reached. Another way of saying this is that when a system that is in equilibrium is disturbed, the system adjusts itself to reduce the change.

For instance, you know that the volume of a gas decreases with increased pressure. So, if you have two volumes of gas in equilibrium, if one volume decreases with increased pressure, the other volume must increase with decreased pressure. Think of it like a teeter-totter. As one side goes up, the other must go down.

## Effect of Change in Concentration

Chemical reactions that are in equilibrium are affected by three different changes: change in concentration of products or reactants, change in temperature, and change in pressure. When one of these changes or 'stressors' is applied to a reaction in equilibrium, the rates of the forward and reverse reactions are no longer equal. The system will change so that either more product or more reactants are made. In time, though, a new chemical equilibrium will be reached, and the forward and reverse reactions will again be equal.

If a chemical reaction in equilibrium has changes in the concentration of the products or reactants, the reaction changes until it comes back into equilibrium. For instance, if you increase the concentration of the reactant, this added stress on the system causes the reaction to make more product, essentially making its forward rate greater than its reverse rate. Since the forward reaction is increasing, the equilibrium is said to shift right. This will continue until the concentration of the reactant has lessened. At this point, the forward and reverse rates will be equal again, and the reaction will be in equilibrium.

## Effect of Change in Temperature

Temperature is also a stress on the reaction system. If a reaction is exothermic, meaning it gives off heat as it proceeds forward, increasing the temperature of the reaction leads to a shift to the left. Therefore, more product is being broken down and more reactant is being made. As product of a usually exothermic reaction is broken down, energy is absorbed, so by making more of the reactants, some of the energy that is added to the system through the increased temperature is then removed.

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