Chemical Processes and Equilibrium

Explore how chemical processes transform reactants into products through energy changes, covering synthesis, decomposition, single and double displacement, combustion, redox, reaction mechanisms, equilibrium, and conservation of mass and energy.

Explore how breaking bonds costs energy and forming bonds releases it, driving exothermic and endothermic reactions. Apply Hess's law and standard enthalpy data to predict energy changes.

Catalysts speed up reactions by providing lower energy pathways without being consumed, enabling homogeneous and heterogeneous forms. Enzymes maximize efficiency, while catalysts power processes like Haber process and catalytic converters.

Collision theory explains reaction rates through collision frequency, energy, temperature, concentration, and orientation, with activation energy and Boltzmann distribution governing effective collisions, while catalysts lower barriers and improve orientation.

Chemical equilibrium occurs when forward and reverse reaction rates are equal, including reversible reactions, keeping concentrations steady in a closed system at constant temperature and pressure.

Construct the equilibrium constant expression from products over reactants with stoichiometric exponents, compare Kc and Kp, use Q and ICE tables, and examine temperature effects via Van't Hoff.

Explore Le Chatelier's principle and how chemical systems counteract disturbances. Learn how concentration, pressure, temperature, and catalysts drive equilibrium shifts with the Haber process and oxygen release to tissues.

Discover how temperature shifts chemical equilibrium by changing the K value, treating heat as a reactant or product, and apply the van't Hoff equation and Le Chatelier principle.

Analyze how equilibrium shifts under pressure using ice tables, partial and total pressures, and Q versus K with disturbances like compression and inert gases. Apply Le Chatelier's principle to scenarios.

Explore acid-base chemistry by identifying acids as proton donors and bases as proton acceptors, and analyze conjugate pairs, hydronium and hydroxide roles, and the pH, Ka, and Kb balances.

Understand solubility equilibrium and the Ksp as the governing constant, with solid activity treated as one, while ion concentrations reflect dissolution, precipitation, and Qsp dynamics.

Explore oxidation-reduction reactions as electron transfers, learn to balance redox equations with the half-reaction method, and connect oxidation states and standard reduction potentials to cell spontaneity.

Explore electrochemical processes that convert chemical energy to electricity, driven by electrodes, electrolytes, and external circuits, including galvanic and electrolytic cells, batteries, and corrosion.

Explore phase equilibrium across solids, liquids, and gases, using phase diagrams, triple and critical points, and Raoult’s, Henry’s, and Clausius–Clapeyron laws to predict vapor pressure and separations.

Discover how equilibrium shapes real-world systems from the Haber process and sulfuric acid production to blood buffering and environmental chemistry, showing how pressure, temperature, and catalysts drive reactions.