🧪 Chemical Equilibrium – At a Glance
🔹 Meaning
Chemical equilibrium is the state in a reversible reaction when the rate of the forward reaction equals the rate of the backward reaction.
🔹 Key Features
The reaction is dynamic (still going on).
Concentrations of reactants and products remain constant.
It occurs only in a closed system.
🔹 Reversible Reaction
A reversible reaction is one that can go both forward and backward.
Example:
N2 + 3H2 ⇌ 3NH3
🔹 Le Chatelier’s Principle
When a system is in equilibrium and it is disturbed by an external constraint the equilibrium will adjust itself so as to oppose the disturbance in order to restore equilibrium.
🔹 Factors Affecting Equilibrium
| Change | Effect |
|---|---|
| Increase in concentration of reactants | Shifts equilibrium to the right |
| Increase in concentration of products | Shifts equilibrium to the left |
| Increase in pressure (gases) | Favors the side with fewer gas molecules |
| Increase in temperature Decrease in temperature | Favors the endothermic reaction Favors the exothermic reaction |
| Catalyst | Does not change equilibrium position |
🔹 Role of a Catalyst
A catalyst alters both forward and backward reactions but does not change the equilibrium position.
🔹 Important Tip
At equilibrium, reactions do not stop — only the rates become equal.
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