Equilibrium Chemistry

Ms. Emmel

What is left our of the Equilibrium expression

Solids, Liquids, liquid water

If K> 1

More products at equilibrium

K< 1

More reactants at equilibrium

If Q < K

There are less products, reaction needs to go forward

Q > K

There are more products, reaction needs to go in reverse

Equilibrium constant is _________ Dependent

Temperature

Equilibrium occurs when the graph ______

Flattens out

Tf we reverse a reaction, the k value is…

1/k (The reciprocal)

If we change the coefficients by multiplying, then …

The original K is raised to the power of the multiplyer

If we add several reactions together then K is …

The product of the individual reactions’ K values

Le Chatelier’s Principle

Changes in concentration, temp or volume/pressure durring equilibrium causes the system to shift to a new equilibrium

Add Reactant at Equilibrium?

Reaction shifts Forward (More products)

Remove Reactant at Equilibrium?

Reaction shifts reverse (More reactants)

Add Product at Equilibrium?

Reaction shifts Reverse (More reactants)

Remove product at Equilibrium?

Reaction Shifts Forward (More product)

In a exothermic Reaction, heat is what ?

A product

In a endothermic reaction, heat is a what?

Reactant

Add heat to an endothermic reaction …

K increasing (Forward)

Remove heat from an Endothermic Reaction . . .

K decreases, (reverse)

Add heat to an exothermic reaction

K Decreases (Reverse)

Remove heat from an Exothermic Reaction . . .

K Increases (Forward)

Increase Pressure

Favors side with Fewer Moles

Decrease Pressure

Favors side with more moles

Increase volume

favors side with more moles

Decrease Volume

Favors side with fewer moles

What do catalysts do when added to a reaction?

They do NOT shift the equilibrium position

What happens when I increase the surface area?

The equilibrium will NOT shift!