Calorimetry and quantitative chemical systems

What this note covers

1. Calorimetry: E = mcΔT and molar enthalpy
2. Worked example: molar enthalpy of combustion and its limitations
3. Quantitative reaction rate from concentration-time data
4. Equilibrium constant expressions and the ICE table
5. Worked example: calculating Kc at equilibrium
6. Using Q to judge equilibrium direction, and pH and Ka links
7. How Section D examines energy, rate and equilibrium calculations, and what separates a top response

7 sections · 11 key terms & formulas · 6 common mistakes