2b.2 - Kinetic Theory Flashcards
What increases the rate of collisions? (3)
- Higher temperature
- Higher concentration
- Larger surface area
Why does a higher temperature increase collisions?
The particles have more energy so they will move at a higher speed so will collide more often
Why does a higher concentration increase collisions?
There are more reactants which makes collisions more likely
Why does a larger surface area increase collisions?
This means the particles around it in the solution will have more area to work on, so there’ll be more frequent collisions
Why are catalysts important for commercial reasons?
They save money because the plant doesn’t need to operate for as long to produce the same amount of stuff
Other than increasing rate of reactions, what else do catalysts do so save money?
Lower activation energy
What are the disadvantages to catalysts? (4)
- Very expensive
- Often need to be taken out and cleaned
- Different reactions use different catalysts
- Catalysts can be ‘poisoned’ so the mixture needs to be kept clean
What is an exothermic reaction?
It gives out energy to the surroundings which results in a raise in temperature
Name three examples of exothermic reactions
- Burning fuels
- Neutralisation reactions
- Oxidation reactions
What is an endothermic reaction?
Takes in energy from the surroundings, which is usually shown by a fall in temperature
Give an example of an endothermic reaction
Thermal decomposition reactions
What type of reactions can be endothermic and exothermic?
Reversible reactions
