Zusammenfassung der Ressource
Rates of Reaction - C2
Anmerkungen:
- 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)
- Ways to change Rate of Reaction
Anmerkungen:
- speed of a reaction= 1/time
- temperature
Anmerkungen:
- 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.
- concentration
Anmerkungen:
- 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
- surface area
Anmerkungen:
- 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
- catalyst
Anmerkungen:
- A catalyst will speed up a reaction without being used up
Anmerkungen:
- 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
- Molar Quantity
Anmerkungen:
- The calculation to see the amount of energy it takes to break the bonds
the energy is measured in KiloJoules (kJ)
- Endothermic and exothermic reactions
Anmerkungen:
- every reaction has 2 parts to it
breaking bonds=endothermic
making bonds=exothermic
- Endothermic Reaction
Anmerkungen:
- Takes in energy from the surroundings
Overall an endothermic reaction gives out less energy making bonds than is taken in breaking bonds
- Exothermic Reaction
Anmerkungen:
- Gives out energy to the surroundings
Overall an exothermic reaction gives out more energy making bonds than is by breaking bonds
- Reversible reactions
Anmerkungen:
- In a reversible reaction the exothermic and endothermic reactions go in opposite directions