Reaction with a smaller equilibrium constant?

In summary, the equilibrium constant (Keq) is a measure of the ratio of products to reactants in a chemical reaction. A larger Keq value indicates a higher ratio of products to reactants, which means that the equilibrium of the reaction lies more on the product side. This is one of the things that the size of Keq can tell us about a reaction.
  • #1
lotsoluv4ya
6
0
How does a reaction with a large equilibrium constant compare to a reaction with a smaller equilibrium constant?
 
Chemistry news on Phys.org
  • #2
Keq=[products]/[reactants] I am sure you probably have seen this before. If the Keq is bigger for one reaction than the Keq for another reaction what does this say about the relationship between the products and reactants for each reaction?
 
  • #3
. . . That the one reaction has a larger ratio of products to reactants than the other reaction . . . I don't know, that's kinda what I was asking you . . .
 
  • #4
Well you kind of just gave yourself the answer. If K is the equilibrium value of the reaction, and something with a larger K has a larger ratio of products to reactants that means that the equilibrium lies more on the right side (product) of the reaction. That is one of the things that the size of K tells you. Where the equilibrium of the reaction lies.
 

1. What is a smaller equilibrium constant in a reaction?

A smaller equilibrium constant in a reaction refers to the ratio of products to reactants at equilibrium. It indicates that the reaction does not favor the formation of products and the reaction may not proceed to completion.

2. How does a smaller equilibrium constant affect the reaction?

A smaller equilibrium constant typically means that the reaction is not favorable and the products are not formed in high quantities. It can also indicate that the reaction is reversible and can proceed in both the forward and reverse directions.

3. What factors can lead to a smaller equilibrium constant?

Factors such as low temperature, high pressure, and low concentrations of reactants can lead to a smaller equilibrium constant. These conditions do not favor the formation of products and can result in an incomplete reaction.

4. Can a smaller equilibrium constant be changed?

Yes, a smaller equilibrium constant can be changed by altering the conditions of the reaction. For example, increasing the temperature, decreasing the pressure, or adding more reactants can shift the equilibrium towards the formation of products and increase the equilibrium constant.

5. How does a smaller equilibrium constant impact the overall yield of a reaction?

A smaller equilibrium constant means that the reaction does not favor the formation of products, which can result in a lower overall yield. This is because not all of the reactants will be converted into products at equilibrium.

Similar threads

Equilibrium and indicator equation
    • Chemistry
Replies
3
Views
859
A question about chemical equilibrium
    • Chemistry
Replies
1
Views
993
Question about equilibrium position
    • Chemistry
Replies
5
Views
2K
Chemical reactions to depict Le Chatelier's Principle (Temperature)
    • Chemistry
Replies
1
Views
1K
Henderson-Hasselbalch equation
    • Chemistry
Replies
8
Views
945
I Equilibrium constant change with stoichiometric doubling (Callen)?
    • Thermodynamics
Replies
5
Views
880
Why does Cu2+ react with I- to give CuI?
    • Chemistry
Replies
7
Views
2K
Interpreting Electrode Potentials
    • Chemistry
Replies
16
Views
3K
Reverse reactions and Le Chateliers principle
    • Chemistry
Replies
3
Views
2K
SO2 Conversion Equilibrium Curve
    • Chemistry
Replies
3
Views
1K

Hot Threads

Recent Insights

Back
Top