8.3Homogeneous & Heterogeneous Catalysts

These flashcards cover the key concepts of homogeneous and heterogeneous catalysts and how they function in chemical reactions.

What is Catalysis?

Catalysis is the process in which the rate of a chemical reaction is increased by adding a substance called a catalyst.

How does a catalyst affect activation energy?

A catalyst provides an alternative reaction pathway that has a lower activation energy than the uncatalyzed reaction.

What is the difference between homogeneous and heterogeneous catalysts?

Homogeneous catalysts are in the same phase as the reactants, while heterogeneous catalysts are in a different phase.

Can you give an example of a homogeneous catalyst?

An example of a homogeneous catalyst could be a situation where both the reactants and the catalyst are liquids.

What is meant by heterogeneous catalyst?

A heterogeneous catalyst is one that is in a different phase than the reactants, such as a solid catalyst acting on gaseous reactants.

What happens to the catalyst during a chemical reaction?

The catalyst is not used up in the reaction and does not appear in the overall chemical equation.

How do catalysts influence the reaction mechanism?

Catalysts allow the reaction to take place through a different mechanism that has a lower activation energy.

What is the significance of the Boltzmann distribution curve in catalysis?

The Boltzmann distribution curve illustrates that catalysts enable a greater proportion of molecules in the reaction mixture to have sufficient energy for effective collisions.

What does a larger shaded area under the curve indicate in catalysis?

A larger shaded area under the curve indicates more particles have energy greater than the activation energy with the catalyst, compared to without it.