Kinetics and Equilibrium

What three things need to happen for a chem reaction to occur

1) Particles must collide

2) Must collide w/ enough force to exceed activation energy

3) Must collide w/ proper positioning

Adding a catalyst

Increases the reaction by lowering the activation energy

Increasing surface area

Increases reaction rate by increasing the number of particles that are able to react

Decreasing temperature

Decreases rate of reaction because particles move slower and collide with less force

Stirring or shaking the reaction

Increases rate of reaction by increasing the number of collisions and energy of them

Adding water to dilute the concentrations

Decreases the rate of reaction by lowering the concentration of substances and decreasing number of collisions

What does the size of Keq tell us about the reaction

Ratio of products to reactants at equilibrium

What is equilibrium

Chem reaction when rate of forward reaction = the rate of the reverse reaction

Constant at equilibrium

Amount of reactants and products

Equal at equilibrium

Speed of forward and reverse reactions

Once the reaction reaches equilibrium does it stop?

No because reactants turning to products and vice versa continue to happen at and equal speed/rate

Add a substance

Away from substance

Decrease substance

Towards that substance

Increase pressure

Side with less gas

Decrease pressure

Side with more gas

Increase volume

Side with more gas

Decrease volume

Side with less gas

Remove solid, add inert gas, add catalyst

No shift

Change temperature

Endo: Heat is a reactant. H is positive

Exo: Heat is a product. H is negative