The following reaction is at equilibrium. N2(g)+ 3H2(g) ⇌ 2NH3(g); Ho= –92kJ Use the Le Chatelier’s principle to predict whether the above equilibrium will shift right, left, or neither affect when each of the following changes occurs. Explain each shift and how it would affect the amount of NH3 at equilibrium? (a) Either H2 or N2 is added to the equilibrium mixture. (b) H2 is removed from the equilibrium mixture. (c) Some of NH3 liquefies or is removed from the mixture; (d) The equilibrium mixture is compressed into a smaller reaction vessel; (e) The temperature of the equilibrium mixture is increased; (f) Argon gas is added to the equilibrium mixture to increase the total pressure of the mixture; (g) A catalyst is added to the equilibrium mixture
The following reaction is at equilibrium.
N2(g)+ 3H2(g) ⇌ 2NH3(g); Ho= –92kJ
Use the Le Chatelier’s principle to predict whether the above equilibrium will shift right, left, or neither affect when each of the following changes occurs. Explain each shift and how it would affect the amount of NH3 at equilibrium?
(a) Either H2 or N2 is added to the equilibrium mixture.
(b) H2 is removed from the equilibrium mixture.
(c) Some of NH3 liquefies or is removed from the mixture;
(d) The equilibrium mixture is compressed into a smaller reaction vessel;
(e) The temperature of the equilibrium mixture is increased;
(f) Argon gas is added to the equilibrium mixture to increase the total pressure of the mixture;
(g) A catalyst is added to the equilibrium mixture
a) Addition of either H2 or N2 shifts the equilibrium towards right.
b) If H2 is removed from the reaction mixture, equilibrium will shifts towards right.
c) If some of NH3 liquefies or is removed from the mixture, equilibrium will shift in forward direction.
d) As n = -ve, If the equilibrium mixture compressed in smaller reaction vessel, the equilibrium shifts in forward direction.
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