Factors that influence chemical equilibrium position

1. Le Châtelier's Principle

• When a system at equilibrium is disturbed, it will adjust to counteract the change and restore equilibrium.
• The position of equilibrium may shift to favour either the forward or reverse reaction.

2. Factors Affecting Equilibrium

2.1 Temperature $(T)$

• Increasing temperature shifts equilibrium towards the endothermic reaction (absorbing heat).
• Decreasing temperature shifts equilibrium towards the exothermic reaction (releasing heat).

2.2 Concentration $(c)$

• Increasing the concentration of reactants shifts equilibrium towards the products.
• Increasing the concentration of products shifts equilibrium towards the reactants.
• Removing a substance from the system shifts equilibrium towards the side that produces more of it.
• Applies to solutions $(aq)$ and gases $(g)$, but NOT solids $(s)$ or liquids $(l).$

2.3 Pressure $(p)$ (For gaseous reactions only)

• Increasing pressure shifts equilibrium towards the side with fewer gas molecules.
• Decreasing pressure shifts equilibrium towards the side with more gas molecules.

2.4 Catalysts

• Speed up the rate of both the forward and reverse reactions.
• Do NOT change the position of equilibrium—only help the system reach equilibrium faster.