Collision Theory

Temperature affects rate of reaction by changing the:
Kinetic Energy
Concentration of reactants affects rate of reaction by changing the:
Number of collisions
Adding a catalyst affects rate of reaction by changing the:
Alignment of collisions
The surface area affects rate of reaction by changing the:
Number of collisions
Higher surface area makes the reaction
Faster
Higher temperature makes the reaction
Faster
Higher concentration makes the reaction
Faster
Adding a catalyst makes the reaction
Faster
Lower temperature makes the reaction
Slower
Lower concentrations makes the reaction
Slower
Less surface area makes the reaction
Slower
The three parts of the collision theory are
Collisions, kinetic energy, proper alignment
The speed of the molecules in a reaction is their
kinetic energy
At higher temperature, molecules have more
kinetic energy
At lower temperature, molecules have less
kinetic energy
At higher concentrations, there are more
molecular collisions
At lower concentrations, there are less
molecular collisions
When the surface area is increased, there are more
molecular collisions
When the surface area is decreased, there are less
molecular collisions
When a catalyst is present, the reactant molecules
Align more
Which reaction would be faster? 10 degrees or 30 degrees?
30 degrees
Which reaction would be faster? Catalyzed or non-catalyzed?
Catalyzed
Which reaction would be faster? A tablet or a powder?
Powder
Which reaction would be faster? Concentrated reactants or dilute reactants?
Concentrated
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