Le Chatelier's Principle Chemical Equilibrium
Haber Process Dynamics for JEE & NEET
System Disturbances
$$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \Delta H$$
Exothermic Reaction ($\Delta H = -92.4$ kJ/mol)
Increasing pressure shifts equilibrium to the side with fewer gas molecules (Right: 4 moles $\rightarrow$ 2 moles).
Exothermic reaction. Heating the system adds energy, shifting the equilibrium Left to absorb it.
Adding reactants shifts right. Adding Inert Gas at constant volume increases total pressure but does NOT shift equilibrium!
Reaction Chamber & Live Graph
⭐ Core Concept
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions (concentration, temperature, pressure), the position of equilibrium shifts to counteract the change to reestablish an equilibrium.
Observe how the Reaction Quotient (Q) temporarily deviates from the Equilibrium Constant (K) when a slider is moved, forcing the visual particles to convert and shift the concentrations bar graph until Q = K again.
Master Chemical Equilibrium
Access comprehensive notes on Equilibrium Constants, Le Chatelier's Principle, and Ionic Equilibrium.
Access Lecture Notes →
No comments:
Post a Comment