Collision Theory (chemija anglų kalba)

• List 4 factors which can increase the rate of a chemical reaction.
• Explain why increasing surface area of a solid increases the rate of reaction.
• Name a method of measuring the rate of a chemical reaction.
• How does a catalyst work?
Answers
• Concentration, pressure, surface area, temperature, catalyst
• Increasing surface area means a greater number of reactant molecules are able to collide with the surface increasing the number of successful collisions.
• Because changing the pressure of a solution has little effect on concentration.
• They need to collide in the correct orientation and with sufficient energy.
• Collision theory
• Activation energy
• Increases the rate of reaction by increasing the energy the molecules have therefore increasing the chance of successful collisions
• Timing mass lost; gas collection; change in colour/precipitation.
• A substance that increases the rate of a reaction without being used up itself.
• Providing an alternative route with lower activation energy
Kinetics
• Learning Objectives:
• The effect of temperature on reaction rates
• How does a catalyst affect activation energy?
• The study of the speed or rate at which chemical reactions occur
Collision theory
• Reactions occur when the particles of reactants collide, provided they collide with a certain minimum kinetic energy.
• For a reaction to occur, the two particles must first collide so that they come into contact with each other. This will happen more often if there are more particles in a given volume.
Collision Theory
• Not all collisions result in a reaction.
• For a collision to be successful, the molecules must have a minimum amount of energy called the ACTIVATION ENERGY
• AND the particles must have the correct orientation.
• What is Activation Energy?
Activation Energy ( )
• The activation energy is the energy barrier that must be overcome in order for a reaction to occur.
• It prevents reactions from taking place spontaneously e.g. burning petrol.
• Ea
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