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Reaction rates and collision theory · A Level Chemistry · Courselo

Courselo

Chemistry
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Physical chemistry: energetics, kinetics and equilibria

Reaction rates and collision theory

Physical chemistry: energetics, kinetics and equilibria · Lesson 4 of 10

Lesson 4 of 10

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Unit 2

Physical chemistry: energetics, kinetics and equilibria

10 lessons · 16 h 45 min of study

Enthalpy changes and calorimetry1 h 30 min of study
Hess cycles, bond enthalpies and lattice energetics2 h of study
Entropy and Gibbs free energy1 h 45 min of study
Reaction rates and collision theoryReading · 0%
Rate equations, orders, mechanisms and Arrhenius treatment2 h 30 min of study

This unit is ≈20% of the Chemistry, across 10 lessons. Full syllabus

Lesson 4 of 10 · Physical chemistry: energetics, kinetics and equilibria

Reaction rates and collision theory

3 quick checks≈2% of the testFoundational: Foundational: the groundwork the rest of the unit builds on

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By the end you’ll be able to

Define rate of reaction in terms of change in concentration of a reactant or product per unit time.
Measure or calculate rate from experimental data, including gas volumes, mass change, colour change, precipitate formation or concentration-time information.
Determine mean rate and estimate initial rate from graphical data using tangents or gradients.

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Adaptive questions on reaction rates and collision theory.

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Dynamic equilibrium and Le Chatelier’s principle1 h 15 min of study

Equilibrium constants Kc and Kp1 h 45 min of study

Acids, bases and pH calculations1 h 45 min of study

Weak acids, buffers and titration curves2 h of study

Solubility product and precipitation equilibria1 h of study

Explain reaction rate in terms of collision frequency, energy of collisions and activation energy.

Explain the effects of concentration, pressure, surface area, temperature and catalysts on rate using collision theory.

Interpret and sketch Maxwell–Boltzmann distributions to show the effect of temperature and catalysts on the number of particles with energy greater than or equal to activation energy.

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