Catalysts

Arrhenius Equation: $\ln k = - \frac{E_{a}}{RT} + \ln A$

KeiannaPineda1B
Posts: 51
Joined: Mon Jun 17, 2019 7:24 am

Catalysts

Can someone please explain how catalysts lower the activation energy of the transition state?

Vincent Leong 2B
Posts: 207
Joined: Fri Aug 09, 2019 12:15 am

Re: Catalysts

that involves more with biology but essentially they bind to the active site of reaction and does something at the molecular level to ease the interaction between reactants.

Miriam Villarreal 1J
Posts: 105
Joined: Sat Aug 17, 2019 12:16 am

Re: Catalysts

In a chemical reaction, the transition state is defined as the highest-energy state of the system. If the molecules in the reactants collide with enough kinetic energy and this energy is higher than the transition state energy, then the reaction occurs and products form. Therefore since this is fairly hard to do the catalyst facilitate this by lowering this energy so that molecules aren't necessarily required to collide with so much kinetic energy

Samuel Tzeng 1B
Posts: 103
Joined: Sat Aug 24, 2019 12:15 am

Re: Catalysts

I think different types of catalysts use different methods to lower the activation energy