Keq = products/reactions
K(eq) = [products] / [reatants].
If there is a reaction
2A + B = 3C + D
The the equilibrium constant is given by
K(eq) = [C]^3*[D] / [A]^2*[B]
NB Note the use of Square Brickets ; this indicates concentration (in chemistry)
NNB The molar ratios become an index/power/exponent number.
NNNB The value of 'K' is only good for a reaction at a given temperature. If the temperature is altered, then the value of 'K' also changes.
Keq=products
reactants
Keq = [Products][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).
Kc is the equilibrium constant of a chemical reaction; Kp is the equilibrium constant of a chemical reaction at constant pressure.
The value of the equilibrium constant K is only influenced by temperature.
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).
C + O ==> COKeq = [CO]/[C][O]
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.