R2

Rate of reaction + Le Châtelier's principle

Collision Theory

Reactant molecules must collide with correct orientation and generate enough energy to successfully react

How does concentration affect rate of reaction?

Increasing concentration raises the number of reactant molecules, leading to more frequent collisions and a higher reaction rate.

How does particle size affect rate of reaction?

Smaller particle size increases surface area, leading to more collisions and a faster reaction rate.

How does pressure affect rate of reaction?

Increasing pressure compresses gas molecules, resulting in more frequent collisions and an increased reaction rate.

How does volume affect rate of reaction?

Increasing volume decreases concentration, leading to fewer collisions and a slower reaction rate.

How does temperature affect rate of reaction?

Increasing temperature provides more energy to particles, resulting in more frequent and energetic collisions, which increases the reaction rate.

How does a catalyst affect rate of reaction?

A catalyst provides an alternative reaction pathway with a lower activation energy, increasing the rate of reaction.

Equilibrium position (right)

Mostly products, high Kc value

Equilibrium position (left)

Mostly reactants, low Kc value

What happens to equilibrium when pressure increases?

Shifts to side with less moles

What happens to equilibrium when pressure decreases?

shifts to side with more moles

What happens to equilibrium when temperature increases?

Shifts to side with higher energy level

What happens to equilibrium when temperature decreases?

Shifts to side with lower energy level

What happens to equilibrium when reactant concentration increases?

Shifts right towards products

What happens to equilibrium when product concentration increases?

Shifts left towards reactants