Rate of Reaction
- Created by: AConfusedDuck
- Created on: 22-11-17 20:19
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- Rate of Reaction
- What?
- Collision Theory
- Reactions need collisions
- Only some collisions create reactions
- "successful collisions"
- More successful collisions = higher Rate of Reaction
- Only some collisions create reactions
- Only some collisions create reactions
- "successful collisions"
- More successful collisions = higher Rate of Reaction
- Reactions need collisions
- Collision Theory
- Factors
- Temperature
- Increased temp = more energy per particle
- Moving faster, so more likely to collide
- Moving faster, so more likely to collide
- Increased temp = more energy per particle
- Catalyst
- Speeds up reaction without being used up.
- Allows particles to react using less energy
- Enzyme
- Biological Catalyst
- Occur Naturally
- Only work on one substrate
- Concentration
- Increased conc = more particles per area
- More particles mean that they are more likely to collide
- Increased conc = more particles per area
- Particle Size
- Decreased particle size = higher surface area
- Higher surface area = higher chance of collision
- Higher surface area = higher chance of collision
- Decreased particle size = higher surface area
- Temperature
- Monitoring RoR
- Change in:
- *Concentration of reactants or products
- *Mass of reactants or products
- *Volume of reactants or Products
- Change in:
- Calculations
- Change in quantity/Change in time
- Rate graphs
- The steeper the line, the faster the rate.
- When the line plateaus, the reaction is over.
- What?
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