Chemistry C6

• The rate = how fast the reactants are changed into particles
• An example of a slow reaction is the rusting or iron and chemical weathering
• An example of a moderate speed reaction is the reaction of magnesium and acid
• An example of a fast reaction is burning and explosions

Collision theory

• The more collisions, the faster the reaction
• The particles must collide with enough energy for the collision to be successful

• As temperature increases, particles move faster
• They collide more frequently
• They have more energy

• More particles in the same volume
• Pressure = same particles in a smaller space
• Collisions are more frequent

• Breaking it into smaller pieces will increase its surface area
• Same volume = more area to work and therefore more collisions

• It decreases the activation energy

• Reactions that can pass both ways through the equilibrium
• As the forward and backward reaction is at the same rate, the system is at equilibrium - 'closed system

• To the right = products greater than reactants
• To the left = reactants greater than products
• These depend on: temperature, pressure, and concentration

• The idea that if you change the conditions of a reversible reaction at equilibrium, the system will try to counteract that change
• It can be used to predict the changes in a system

• When the reaction increases, the equilibrium will act in the opposite way to try and decrease it
• When the reaction decreases, the equilibrium will act in the opposite way to try and increase it