Understanding Redox Reactions and Chemical Equilibrium

This comprehensive page covers fundamental concepts of oxidation-reduction reactions and chemical equilibrium calculations. The content explains electron transfer processes and methods for balancing chemical equations.

Definition: Oxidation is defined as the loss of electrons, while reduction is the gain of electrons in a chemical reaction.

Vocabulary:

• Oxidizing agent (Oxidant): Chemical species capable of accepting one or more electrons
• Reducing agent (Reducteur): Chemical species capable of donating one or more electrons

Highlight: The method for balancing redox equations involves several key steps:

1. Separate oxidizing and reducing agents
2. Account for stoichiometry excluding hydrogen and oxygen
3. Add H2O molecules to conserve oxygen
4. Add H+ ions to conserve hydrogen
5. Balance charges by adding electrons (e-)

Example: The formation of copper(II) hydroxide is demonstrated through the equation: Cu²⁺(aq) + 2OH⁻(aq) → Cu(OH)₂(s)

Definition: The progress table (tableau d'avancement) shows:

• Initial state (état initial)
• Intermediate state (état intermediaire)
• Final state (état final) tracking the molar quantities of reactants and products throughout the reaction.