K>1 vs K<1
Moderators: Chem_Mod, Chem_Admin
-
Kelly McBratney 1C
- Posts: 23
- Joined: Fri Sep 25, 2015 3:00 am
K>1 vs K<1
How come when K>1 (there is a higher concentration of products than reactants), the reaction favors the products? I would have thought that because there are more products, the reverse reaction would be favored in order to balance the products and reactants.
-
Chem_Mod
- Posts: 23858
- Joined: Thu Aug 04, 2011 1:53 pm
- Has upvoted: 1253 times
Re: K>1 vs K<1
You may be confusing Q with K. Remember K is the ratio of products to reactants at equilibrium and it can be any positive number from 0 to near infinity.
Q<K means there is a lack of products and will shift to make more products
Q>K means there is too many products and will shift back to reactants
Q<K means there is a lack of products and will shift to make more products
Q>K means there is too many products and will shift back to reactants
Return to “Gibbs Free Energy Concepts and Calculations”
Who is online
Users browsing this forum: No registered users and 7 guests