Topic 16 Kinetics

The rate is proportional to the concentration of a reaction Rate equation: Rate = k[A]^1

The rate is proportional to the square of the concentration Rate equation: Rate = k[A]^2

Increasing concentration has no effect on rate Rate equation: Rate = k[A]^0 Therefore in a zero order reaction, the rate is equal to the rate constant.

The overall rate of reactants is the change in concentration of a species divided by the time taken for the change to occur. All reactions rates are positive. Rate = d[product]/dt Rate = -d[reactant]/dt

When a gas is involved look for (g) in equation

When a coloured species is lost or produced we can measure the loss/gain in intensity of that colour (halogens are common examples)

When a relatively dense gas such as CO2 is evolved

Quench the reaction, then titration to obtain the concentration of a species. Often used when acids are involved, either as reactants/products or catalysts.

When an increase/decrease in the number of ions occurs in the reaction

Rate = change in concentration/time

mol dm^-3 s^-1

Increasing temperature –> increased rate of reaction Much higher proportion of particle have energy greater than the activation energy = many more successful collisions.

Use a flash of light to break bonds, use probe flashes to record amount of light absorbed by a species. This can show its concentration.

e^(ΔG/-RT)