Hello fellow chemists,
I've been studying chemical equilibrium and came across a reaction where the equilibrium constant expression seems a bit complex. The reaction is as follows:
$$\text{aA} + \text{bB} \rightleftharpoons \text{cC} + \text{dD}$$
Given that the stoichiometric coefficients are integers, how would you derive the expression for the equilibrium constant ( K )? Additionally, how does the change in concentration of one of the reactants affect the equilibrium position?
Understanding the Equilibrium Constant Expression
Moderators: Xen, expert, ChenBeier
-
- Newbie
- Posts: 1
- Joined: Fri Apr 05, 2024 12:40 am
- ChenBeier
- Distinguished Member
- Posts: 1570
- Joined: Wed Sep 27, 2017 7:25 am
- Location: Berlin, Germany
Re: Understanding the Equilibrium Constant Expression
Law of mass action
K = C^c*D^d/(A^a*B^b)
K = constant, so changes of one component will affect all others.
https://www.chemistrylearner.com/law-of ... ction.html
K = C^c*D^d/(A^a*B^b)
K = constant, so changes of one component will affect all others.
https://www.chemistrylearner.com/law-of ... ction.html