Catalyst increasing both forward and reverse reaction rate

In summary, when a catalyst is added to a reaction at equilibrium, the forward and reverse reaction rates are increased equally. This is because the catalyst increases the concentration of both reactants and products, leading to an increase in the rates of both the forward and reverse reactions. This phenomenon is known as dynamic equilibrium, where the reaction continues to occur in both directions at equal rates.
  • #1
TT0
211
3
Please post this type of questions in the HW section using the template.
The question is:

Which takes place when a catalyst is added to a reaction at equilibrium?

A. The point of equilibrium is shifted to the right.
B. The point of equilibrium is shifted to the left.
C. The forward and reverse reactions rates are increased unequally.
D. The forward and reverse reactions rates are increased equally.
E. The value of ΔH has the same magnitude but a different sign.

I chose C because I think that a catalyst would increase the reaction rate of one way. The other way would also increase a bit because of the increased concentration of it. However, the answer is D, they both increase equally. I don't understand how this is possible, could someone explain this?

Thanks
 
Physics news on Phys.org
  • #2
It gets where it's going faster.
 
  • Like
Likes TT0

What is a catalyst?

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It works by providing an alternative pathway for the reaction to occur with a lower activation energy, making the reaction more likely to happen.

How does a catalyst increase the forward reaction rate?

A catalyst increases the forward reaction rate by lowering the activation energy required for the reaction to occur. This allows the reactant molecules to overcome the energy barrier more easily and proceed with the reaction at a faster rate.

How does a catalyst increase the reverse reaction rate?

A catalyst increases the reverse reaction rate by providing an alternative pathway for the reverse reaction to occur with a lower activation energy. This means that the products can more easily revert back to the reactants, increasing the rate of the reverse reaction.

Does a catalyst affect the equilibrium of a reaction?

Yes, a catalyst can affect the equilibrium of a reaction by increasing both the forward and reverse reaction rates. However, it does not shift the position of the equilibrium, meaning the amount of products and reactants at equilibrium will remain the same.

What are some examples of catalysts?

Some common examples of catalysts include enzymes in biological reactions, transition metals like platinum or nickel in industrial reactions, and acids or bases in chemical reactions. These substances can increase the rate of a wide range of reactions without being consumed themselves.

Similar threads

Chemistry Finding rate constant from pressure change in an experiment
    • Biology and Chemistry Homework Help
Replies
2
Views
1K
Factors Affecting the Rate of Reactions
    • Biology and Chemistry Homework Help
Replies
2
Views
8K
Increase Catalyst Surface Area & Reaction Rate: Experiment
    • Biology and Chemistry Homework Help
Replies
3
Views
2K
Reaction rates, temperature, and thermal energy
    • Biology and Chemistry Homework Help
Replies
5
Views
1K
Engineering Tubular Reactor with catalytic walls
    • Engineering and Comp Sci Homework Help
Replies
6
Views
772
Deriving a Rate Equation for a Reversible Elementary Mechanism
    • Biology and Chemistry Homework Help
Replies
15
Views
3K
Chemical reactions to depict Le Chatelier's Principle (Temperature)
    • Chemistry
Replies
1
Views
1K
Increasing Yield of a System with Le Chatelier's Principle
    • Biology and Chemistry Homework Help
Replies
5
Views
2K
Proposing a reaction mechanism
    • Biology and Chemistry Homework Help
Replies
10
Views
4K
Question about equilibrium position
    • Chemistry
Replies
5
Views
2K

Hot Threads

Recent Insights

Back
Top