Le Chatelier’s Principle: Heat & Enthalpy
Exothermic Reaction
A + B → AB + Heat
Heat Released
Endothermic Reaction
A + B + Heat → AB
Heat Absorbed
298 K
System Status: Initializing… | KC: Calculating…
A (Reactant)
B (Reactant)
AB (Product)
Enthalpy (ΔH)
Activation Energy
Understanding Heat and Enthalpy in Chemical Equilibrium
Exothermic Reaction: Releases heat (ΔH < 0). Increasing temperature shifts equilibrium toward reactants.
Endothermic Reaction: Absorbs heat (ΔH > 0). Increasing temperature shifts equilibrium toward products.
Key Observations:
- Temperature changes affect the equilibrium position differently for exo- and endothermic reactions
- The energy diagram shows relative energy levels of reactants and products
- Catalysts lower activation energy but don’t affect equilibrium position or ΔH
- KC changes with temperature but not with concentration or catalyst
Current KC = [AB] / ([A] × [B]): 0
Enthalpy Change (ΔH): 0 kJ/mol