A catalyst basically allows an intermediate step in a chemical reaction.
Every reaction has an activation energy that is required to start it, wich means a certain temperature is needed to make the reaction happen fast (since temperature is randomly distributed “too cold to react” means a few molecules will still react randomly, but that will be slow)
A catalyst basically splits that energy required by doing the reaction in two steps. Like, imagine instead of having to climb a 4 feet step you have to do 2 feet twice wich is much easier.
This results in much lower temperature being needed for a fast reaction.
So your chemical reacts with platinum, and that then reacts to the final result releasing the platinum again.
Random funfact: our body relies heavily on enzymes that work like catalysts. That way we can burn our food at body temperature and not at fat-fire temperature.
~~The super dimple version is, if your trying to light a burn pile on fire, gasoline acts as a catalyst. Catalysts make things happen “more”. Whether faster, cheaper, easier, skipping a step, skipping an ingredient. Catalysts just allow things to happen that would normally require an additional something. Even if that something is “more of this thing you already have”.~~
it has been explained that i am wrong, so please listen to the people smarter than me.
Catalysts speed up a reaction by lowering the activation energy. This is done by stabilising the intermediate steps in the reaction.
Transition metal catalysts like platinum work by letting chemicals “borrow” some electrons for a while and letting them sit on the surface of the metal waiting for the other reagent to come along and react.
Latest Answers