Rates of Chemical Reactions
- Created by: victoriarevision
- Created on: 01-04-16 13:39
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- Rates of Chemical Reactions
- Temperature
- Molecules must collide with activation energy.
- Higher temperatures mean more particles have enough energy to react.
- Higher temperatures mean particles move faster. Hence there are more collisions.
- Pressure
- Higher pressure means the same number of particles in a smaller volume.
- Increasing pressure increases the chance of more frequent collisions.
- Increasing pressure increases the collisions with enough energy to react.
- Concentration
- Higher concentration means more particles in the same volume.
- Increasing the concentration increases the chance of more frequent collisions.
- Increasing the concentration increases the collisions with enough energy to react.
- Surface Area
- Increasing surface area increases the chance of more frequent collisions.
- Increasing surface area increases the collisions with enough energy to react.
- Addition of a Catalyst
- A catalyst increases the rate of reaction without being used in the reaction.
- Catalysts lower the activation energies for reactions.
- Orientation
- If the orientation of the particles is not correct no reaction will occur.
- Particles must collide head on in order to overcome the activation energy.
- Calculating Rates of Reactions
- To calculate rate changes in physical quantities must be measured.
- Change in mass
- Gas volume
- Concentration
- Other: colour, conductivity, pressure
- The physical changes can be drawn on a graph.
- To find the rate draw a tangent to the curve and calculate its gradient.
- To calculate rate changes in physical quantities must be measured.
- Temperature
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