A11.1 Principles of Collision Theory

Activation energy, successful and unsuccessful collisions, and why particles must meet in the correct spatial orientation.

Learning outcomes

• Explain why reacting particles must collide
• Define activation energy
• Distinguish successful and unsuccessful collisions
• Explain correct spatial orientation

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More T-Level Chemistry topics

A11.2 Temperature and Rate of ReactionHow temperature changes kinetic energy, collision frequency and the Maxwell–Boltzmann distribution, and why rate rises or falls.A11.3 Catalysts and Reaction RateWhat a catalyst is, the alternative lower-Ea pathway, and how that appears on a Maxwell–Boltzmann distribution at constant temperature.A12.1 Factors Affecting Rates of Chemical ReactionsSurface area, concentration and pressure explained with collision theory. The PowerPoint 95 s / 48 s times and the workbook 96 s / 51 s / 29 s times are kept separate.A12.2 Calculating Rate of ReactionAverage rate from amount of reactant used or product formed divided by time, including compound units and graph chords.A12.3 Enthalpy ChangesH and ΔH, exothermic and endothermic profiles, activation energy, and why a catalyst does not change ΔH.A12.4 Catalysts in Industrial ReactionsLower activation energy, faster industrial turnaround and reduced costs, with unchanged ΔH.A12.5 Reversible ReactionsDynamic equilibrium and Le Chatelier’s principle for concentration, temperature and pressure.A12.6 The Haber ProcessTypical Haber conditions and the compromise between equilibrium yield, rate and economic cost.

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