Rates Of Reaction Flashcards
Particle collision theory
For a chemical reaction to occur, particles must collide with sufficient energy to overcome the energy
Increasing temperature
More frequent successful collisions as more particles have enough KINETIC energy to overcome the activation energy
Increasing concentration
More reactant particles per volume, so there will be more frequent collisions
Increasing surface area
More opportunities for collisions to occur so more frequent successful collisions
What does a catalyst do
Increases the rate but is not chemically changed or used up during the reaction
Adding a catalyst
A catalysed reaction requires less energy to occur so they are more frequent successful collisions
How does a catalyst work
By providing an alternative pathway with lower activation energy
What is the activation energy
The minimum amount of energy needed for the particles to react
Surface area practical
Marble chips in hydrochloric acid and how much gas is produced- change size of marble chips eg. powder
Concentration practical
Marble chips and hydrochloric acid and how much gas is produced - change concentration of acid
Temperature practical
Sodium thiosulfate solution and hydrochloric acid and how long it takes for the cross to disappear- different temperature water baths
Catalyst practical
Add solids to hydrogen peroxide solution and calculate the amount of solid left at the end of the reaction. Best solid caused bubbles and wasn’t used up
