The chemical reactions which takes place in both Such equilibrium is established in physical reactions.
directions are called reversible reactions It is dynamic in nature.
Equilibrium is the end state of a reversible reaction.
Gaseous Equilibrium is established only in a closed container.
Here vapour pressure is constant at a constant temp for given.
At equilibrium, the rate of forward and backward
reactions are equal.
At equilibrium, the concentration of reactants & Established only at a constant temparature
products becomes constant. o
Ice-water equilibrium established at 0 C (at1atm)
Established only in a Saturated solution
eg: Saturated sugar solution.
Sugar (dissolved) Sugar (undissolved)
Equilibrium
forward
product
equilibrium
Rate Conc Here solubility depends upon pressure (Henry’s law)
reactant eg: Soda water
backward
CO (dissolved) CO (undissolved)
Time Time
Q. For the equilibrium A B, the variation of the rate of the forward (a) & Q. Which of the given statements does not elucidate the equilibrium state Q In
reverse (b) reaction with time is given by precisely? of
(A) The equilibrium can be approached from either direction.
(B) The equilibrium can be attained only if the system is an isolated system. (A
(C) The free energy change at constant pressure and temperature is zero.
(D) It is dynamic in nature.
CHEMICAL EQUILIBRIUM
Applications of K & Q
• Value of K depends only on temperature.
• If K for the reaction aA + bB cC+dD is K, then
K for the reaction cC+dD aA+ bB will be K1 If they are in solid or liquid phase(or aqueous), K can be represented as Kc.
If they are in gaseous phase, K can be represented as Kp
• If K for the reaction aA + bB cC+dD is K, then
For a general reaction
K for the reaction naA+ nbB ncC + ndD will be (K)n
aA + bB cC + dD
• During the addition of two reactions having equilibrium [C]C [D]d PCc PDd
constants K & K2, then the net Constant K = K x K Kc = & Kp =
[A] [B]
a b PAa PBb
• During the subtraction of a reaction having constant K from a
reaction having constant K , then the net constant K = K /K Kp = Kc (RT) n g ng = np - nR
directions are called reversible reactions It is dynamic in nature.
Equilibrium is the end state of a reversible reaction.
Gaseous Equilibrium is established only in a closed container.
Here vapour pressure is constant at a constant temp for given.
At equilibrium, the rate of forward and backward
reactions are equal.
At equilibrium, the concentration of reactants & Established only at a constant temparature
products becomes constant. o
Ice-water equilibrium established at 0 C (at1atm)
Established only in a Saturated solution
eg: Saturated sugar solution.
Sugar (dissolved) Sugar (undissolved)
Equilibrium
forward
product
equilibrium
Rate Conc Here solubility depends upon pressure (Henry’s law)
reactant eg: Soda water
backward
CO (dissolved) CO (undissolved)
Time Time
Q. For the equilibrium A B, the variation of the rate of the forward (a) & Q. Which of the given statements does not elucidate the equilibrium state Q In
reverse (b) reaction with time is given by precisely? of
(A) The equilibrium can be approached from either direction.
(B) The equilibrium can be attained only if the system is an isolated system. (A
(C) The free energy change at constant pressure and temperature is zero.
(D) It is dynamic in nature.
CHEMICAL EQUILIBRIUM
Applications of K & Q
• Value of K depends only on temperature.
• If K for the reaction aA + bB cC+dD is K, then
K for the reaction cC+dD aA+ bB will be K1 If they are in solid or liquid phase(or aqueous), K can be represented as Kc.
If they are in gaseous phase, K can be represented as Kp
• If K for the reaction aA + bB cC+dD is K, then
For a general reaction
K for the reaction naA+ nbB ncC + ndD will be (K)n
aA + bB cC + dD
• During the addition of two reactions having equilibrium [C]C [D]d PCc PDd
constants K & K2, then the net Constant K = K x K Kc = & Kp =
[A] [B]
a b PAa PBb
• During the subtraction of a reaction having constant K from a
reaction having constant K , then the net constant K = K /K Kp = Kc (RT) n g ng = np - nR
