⚖️ Le Chatelier's Principle Equilibrium Simulator
EquilibriumWhat's happening? N₂ + 3H₂ ⇌ 2NH₃. Increase pressure → shifts to fewer moles (right). Increase temperature → shifts to endothermic direction. This is Le Chatelier's principle in action.
Equilibrium: 8-10 questions every year.
JEE tests Kp, Kc, pressure/concentration/temperature effects, Q vs K.
Key formulas
Le Chatelier's Principle Formulas
K_c
K_c = [C]^c[D]^d / [A]^a[B]^b
Products over reactants
Kp-Kc
K_p = K_c(RT)^Dn
Dn = gas moles change
Q
Q = same form as K
Q
Van t Hoff
ln(K2/K1) = -dH/R(1/T2-1/T1)
K vs temperature
Step-by-step problem solving
How to solve chemistry problems in JEE
- Write balanced equation and K expression
- Identify given values
- Calculate Q if not at equilibrium
- Apply Le Chatelier for P, C, T changes
Common JEE mistakes
What students get wrong
Solids in K
Only gases and aqueous in K. Solids/liquids omitted.
Wrong Dn
Dn = gas products - gas reactants
Temperature effect
Increase T favors endothermic
Q vs K
K at equilibrium, Q at any time
FAQs
Le Chatelier's Principle Questions
Pressure increase effect?
Shifts to fewer gas moles side.
Catalyst changes K?
No. Speeds both directions equally.
Temperature effect on K?
Exothermic: T up, K down. Endothermic: T up, K up.
Q = K?
Yes, at equilibrium.