Molarity of products divided by reactants
Keq=(products)/(reactants)
The Keq is a ratio of the concentrations of products to reactants at equilibrium. So, one way to determine it would be to measure the concentrations of all species at equilibrium (when concentrations are no longer changing). aA + bB <--> cC + dD and Keq = [A]^a[B] ^b/[C]^c[D]^d
There is no answer here so why the heck even try to comment
k=[A+][Q-]/[AQ]
these measurements must be taken at saturation of course.
The equilibrium constant of a chemical reaction is determined experimentally or by computational methods.
The equilibrium constant can tell us how the reaction is going. If the constant is grater than one there are more products than reactants, so the reaction os closer to completion. If the equilibrium constant is less than 1 it shows that there are a lot more products than reactants so the reaction has not really started yet.
At equilibrium the concentrations of reactants and productas remain constant.
It is the ratio of the concentrations of products to the concentrations of reactants.
It is the ratio of the concentrations of products to the concentrations of reactants.
It is the ratio of the concentrations of products to the concentrations of reactants.
The molarity of products is divided by the molarity of reactants
Kc is the equilibrium constant of a chemical reaction; Kp is the equilibrium constant of a chemical reaction at constant pressure.
An equilibrium constant
An equilibrium constant
Kb= 1/Kf (:
If the equilibrium constant is zero, the reaction canNOT (will NEVER) reach equilibrium, it can not react back because all products are 'removed' (= concentration is zero).
The reaction proceeds to a very large extent if Kc >> 1. On the other hand, the reaction hardly proceeds if Kc << 1.
A small equilibrium constant value means equilibrium will never establish or the amount of products in reaction mixture is negligible.
Equilibrium constant changes when temperature changes. For an endothermic reaction, the equilibrium constant increases with temperature while for an exothermic reaction equilibrium constant decreases with increase in temperature. Equilibrium constants are only affected by change in temperature.
It tells whether products or reactants are favored at equilibrium
When a chemical reaction reach the equilibrium she can not continue spontaneously.
Law of equilibrium - The principle that (at chemical equilibrium) in a reversible reaction the ratio of the rate of the forward reaction to the rate of the reverse reaction is a constant for that reaction.