Thermochemistry Workbench
Guided thermochemistry lessons for calorimetry, formation enthalpy, Hess’s law, bond energies, heating curves, entropy, Gibbs energy, catalysts, fuels, and temperature corrections.
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How this tool works
Eleven guided modules connect experimental temperature changes and tabulated data to reaction energy, spontaneity, equilibrium, and kinetic barriers.
Every module states a chemical question, learning objective, observations, governing relationship, and practice challenge.
Diagrams use labeled units and explain what the current result means rather than displaying an isolated number.
Core equations
q = mcΔT and q_rxn = −q_surroundingsΔH°rxn = ΣνΔH°f(products) − ΣνΔH°f(reactants)ΔH ≈ ΣD(bonds broken) − ΣD(bonds formed)ΔS°rxn = ΣνS°(products) − ΣνS°(reactants)ΔG = ΔH − TΔS and ΔG° = −RT ln KΔH(T₂) ≈ ΔH(T₁) + ΔCp(T₂ − T₁)Assumptions
- Coffee-cup calorimetry is treated as approximately constant pressure with negligible external heat loss.
- Bomb calorimetry reports constant-volume internal-energy change.
- Bond enthalpies are average gas-phase values and provide estimates.
- Gibbs and equilibrium calculations use the entered standard-state thermodynamic values.
- Kirchhoff correction assumes a constant reaction heat-capacity difference over the temperature interval.
Limitations
- The diagrams are conceptual and not molecular-dynamics simulations.
- Real calorimeters require calibration, heat-loss correction, and uncertainty analysis.
- Thermochemical data must use compatible reference states, units, and balanced stoichiometry.
- The tool is educational and does not replace laboratory safety procedures or validated process design.