Below are a number of misconceptions in the Reaction Rates section of the course. For each misconception, I've given a description and example for how we can combat such devious cisconceptions!
- Equilibrium is the state where the rates of the forward and reverse reactions are equal, not when the rates reach zero.
- Common misconception: Nothing is happening at equilibrium.
- Common misconception: Nothing is happening at equilibrium.
- The reaction rate is constant!
- The reaction rate can vary widely! We have multi-step reactions like the Iodine-Clock Reaction!
- A catalyst will increase the amount of possible product!
- A catalyst will simply help the reaction proceed to the products but does not add the the yield!
- There must be more than one reactant in the reaction!
- There are many reactions involving a single reactant! Think of graphene sheets being made from pure graphite!
- Cooling down a reaction can aide it in going faster too!
- In very rare cases is this true, but for the large majority of reactions it will only slow it down!
The following video shows that there are many misconceptions in science!