Reaction Rates

How fast a reaction is

How big a reaction is

How loud a reaction is

How much gas a reaction produces

Chemical Energy

Kinetic Energy

Activation Energy

Potential Energy

Carbonic energy

Activation energy

Plutonic energy

Resting energy

taken in

given out

The energy needed for a reaction to occur

The minimum amount of energy needed for a reaction to potentially occur

The energy added by a catalyst

The energy possessed by the products

the particles also need to collide with a catalyst

not all the particles collide with enough energy

not all the particles collide at a high enough temperature

the particles need to collide with each other twice

When molecules collide.

When molecules collide with the proper orientation.

When molecules collide with proper orientation and enough kinetic energy.

High Temperature.

Catalyst

Acid

Base

pressure

concentration

surface area

temperature

reactants

it increases both the frequency and energy of particle collisions

it only increases the frequency of particle collisions

it only increases the energy of particle collisions

it reduces the activation energy of the reaction

it increases the amount of reactants

it lowers the activation energy

it increases the energy of particle collisions

it increases the frequency of particle collisions

Particles collide more often

Particles collide with more energy

Particles move faster

More particles collide in the correct orientation

Red, because the activation energy is larger

Blue, because the activation energy is lower

both reaction progress at the same rate

By lowering the activation energy or reaction

by giving them more energy

by making them more available

to slow down

to move faster

have proper orientation

hit in the right order

temperature

concentration

surface area

volume

catalysts