Term | Definition |
Activation Energy | the amount of energy needed in order for particles to react when they collide. |
2 things that affect reaction rate | frequency of collisions
amount of energy with which they collide |
5 things that affect frequency of collisions and the amount energy in a reaction | temperature, pressure, surface area, concentration, catalyst |
As a reaction progresses the rate decreases because why? | The reactants are getting used up and the products being produced are interfering with the collisions |
In order for a reaction to take place, the particles must ________________ with each other. | collide |
What does a catalyst do that changes the reaction rate? | It lowers the activation energy |
What are some examples of how catalysts are used in industry? | Catalytic converter, margarine production, laundry detergent |
Is a catalyst an active reactant in a reaction? | No, it remains unchanged |
If the temperature is raised the reaction rate will ________. | Increase |
If the pressure is decreased the reaction rate will ______. | decrease |
As a reaction takes place, the reactants are getting used up and the products being produced are interfering with the collisions, what does this mean for the reaction rate? | It will slow down and eventually stop when the product is at 100%. |
What did the breathe fire lab demonstrate? | That increased surface area increases the reaction rate. |
What did the water to oil lab demonstrate? | That some reactions can seemingly take place in an instant |
What did the elephant toothpaste lab demonstrate? | The use of a catalyst can increase the reaction rate greatly and can produce heat. (Exothermic) |