Define the rate of reaction as the change in concentration of a particular reactant/product per unit time. Determine rates of reaction. Calculation of reaction rates from tangents of graphs of concentration, volume, or mass against time.
Explain the relationship between the kinetic energy of the particles and the temperature in Kelvin, and the role of collision geometry.
Recall the factors that influence the rate of a reaction, including: pressure, concentration, surface area, temperature, and the presence of a catalyst. Predict and explain the effects of changing conditions on the rate of a reaction.
Define activation energy,Ea, as the minimum energy that colliding particles need for a successful collision leading to a reaction. Construct Maxwell-Boltzmann energy distribution curves to explain the effect of temperature on the probability of successful collisions.
Recall that catalysts increase the rate of reaction by providing an alternative reaction pathway with lowerEa. Sketch and explain energy profiles with and without catalysts for endothermic and exothermic reactions. Construct Maxwell-Boltzmann energy distribution curves to explain the effect of different values forEaon the probability of successful collisions.