# Rates of Reaction - C2

Mind Map by jasmine turner, updated more than 1 year ago
 Created by jasmine turner about 5 years ago
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AQA GCSE

## Resource summary

Rates of Reaction - C2

Annotations:

• Atoms must collide in order to react, but they need energy for the collision to be successful (particles in solids don't have enough energy to collide)
1 Ways to change Rate of Reaction

Annotations:

• speed of a reaction= 1/time
1.1 temperature

Annotations:

• As you increase the temperature, you increase the amount of kinetic energy in the particle more energy means more movement, increasing the chance of a collision, increasing the rate of reaction.
1.2 concentration

Annotations:

• with a higher concentration, there are more particles in a set amount of space. more particles mean more collisions in a set time, which leads to a faster rate
1.3 surface area

Annotations:

• as you decrease particle size, you increase surface area more surface area means more chance of a sucessful collision which leads to a faster rate of reaction
1.4 catalyst

Annotations:

• A catalyst will speed up a reaction without being used up
1.4.1

Annotations:

• it provides a surface for the reaction This also lowers the activation energy (energy required to start a reaction)  more likely that the collision is sucessful
2
3 Molar Quantity

Annotations:

• The calculation to see the amount of energy it takes to break the bonds the energy is measured in KiloJoules (kJ)
4 Endothermic and exothermic reactions

Annotations:

• every reaction has 2 parts to it breaking bonds=endothermic making bonds=exothermic
4.1 Endothermic Reaction

Annotations:

• Takes in energy from the surroundings Overall an endothermic reaction gives out less energy making bonds than is taken in breaking bonds
4.2 Exothermic Reaction

Annotations:

• Gives out energy to the surroundings Overall an exothermic reaction gives out more energy making bonds than is by breaking bonds
4.2.1
4.3 Reversible reactions

Annotations:

• In a reversible reaction the exothermic and endothermic reactions go in opposite directions
4.3.1

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