Rate of reaction Flashcards
Particles have to _________ to __________
Particles have to collide to react.
Why does a graph go horizontal and stop at the end of the graph?
The reaction finishes as there is no reactant to react with because it has been used up.
Rate = ________ / _____
Rate = amount of co² / time
What can change the rate of reaction?
- Concentration
- Temperature
- Surface area
- A catalyst
- Pressure
- light
How could the reliability of results be improved?
By repeating the experiment
What is Activation Energy?
Activation Energy is the amount of energy that particles need in order to react together, to start breaking bonds.
The steeper the ______ the _____ the rate of reaction.
The steeper the gradient the faster the rate of reaction.
Give an example of a catalyst:
- Potato peel
- Blood
- MnO²
Energy is used to________
Energy is used to break bonds.
If there is not enough _____ the particles can’t collide.
If there is not enough energy the particles can’t collide.
The more successful the collisions the _____ ____ _____ __ _______.
The more successful the collisions the faster the rate of reaction.
How can rate of reaction can be measured?
By measuring the gas produced in a syringe.
Reducing the size of particles increases the rate of reaction because ………
it increases the surface area available for collisions to take place.
Give an example of a Higher/ Faster rate of reaction:
When petrol is ignited it combines with oxygen and there is almost an instant reaction.
Give an example of a Lower rate of reaction:
Iron rust in air this is a slow reaction.
