equilibrium

Introduction to Equilibrium in Chemical Systems

• Understanding the concept of equilibrium in the context of acids and bases.
• Overview of an anticancer platinum compound as an example of complex chemical interactions.

The Role of Temperature in Equilibrium

• Equilibrium Concentrations: Concentrations of products and reactants remain constant at equilibrium.
• The importance of temperature: Heating a solution can shift the equilibrium depending on the enthalpy change.
  • Example: Mixtures of nitrogen dioxide (NO₂) and dinitrogen tetroxide (N₂O₄), adjusting temperature affects the concentration of these compounds.

Experiments with Gas and Color Changes

• Demonstration using nitric oxide (NO) and dinitrogen tetroxide (N₂O₄):
  • Observation: Two test tubes with reacting gases were placed in hot and cold water respectively.
  • Result: Hot water tube (higher temperature) contained more NO₂ (darkened color) while the cold water tube contained more colorless N₂O₄.
• Implications of color change indicate shifts in equilibrium:
  • Heating shifts equilibrium towards more reactive components, increasing concentration of dark NO₂.
  • Cooling did the opposite, shifting equilibrium towards the lighter N₂O₄.

Le Châtelier's Principle

• Definition: If a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance.
• Examples include:
  • Adding/removing reactants or products changes equilibrium concentrations.
  • Physical changes (like temperature) can alter how an equilibrium is established.

Visual Demonstrations of Equilibrium

• Using colored solutions containing copper ions (Cu²+) to demonstrate complexation:
  • Demos included creating different colored layers by