IP Chemistry Upper Sec 09: Chemical Energetics
26 Nov 2025, 00:00 Z
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Practical course certificate note
For practical, lab, and experiment courses, Eclat Institute may issue an internal Certificate of Completion/Attendance based on participation and internal assessment.
- This is an internal centre-issued certificate, not an MOE/SEAB qualification or accreditation.
- Recognition (if any) is determined by the receiving school, institution, or employer.
- For SEAB private candidates taking science practical papers, SEAB states you should either have taken the subject before or complete a practical course before the practical exam date.
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These notes align with SEAB GCE O-Level Chemistry (6092) content used in IP programmes (exams from 2026).
Status: SEAB O-Level Chemistry 6092 syllabus (exams from 2026) checked 2025-11-30 - scope unchanged; remains the reference for this note.
What you must know
- Enthalpy change is heat change at constant pressure; exothermic releases heat (ΔH < 0), endothermic absorbs heat (ΔH > 0).
- Energy profile diagrams must show relative energy of reactants/products, activation energy peak, and ΔH arrow.
- Bond breaking is endothermic; bond making is exothermic; overall ΔH is “energy to break − energy released making.”
- Qualitative bond-energy comparisons explain why combustion is strongly exothermic and why thermal decompositions need heating.
Detailed notes
- Sign convention: exothermic transfers heat to surroundings (temperature rises), ΔH negative; endothermic absorbs heat (temperature falls), ΔH positive.
- Calorimetry (qualitative at IP): measure mass of solution, temperature change; assume density 1 g/cm³ and specific heat capacity . Identify limiting reagent when expressing ΔH per mole.
- Hess’ idea (qualitative): total enthalpy change is path independent; can use known combustion/formation data to deduce unknown ΔH.
