5.1.1 - How fast

The power to which a conc. of a reactant is raised to in the rate equation

Slightly downward slope (conc vs. time graph) Drops w/ a constant half life Rate=conc; diagonal line in rate vs. conc graph

Decline steeply then level off Parabola in rate vs. conc graph

Rate is proportional to the square of the con. (upward slope)

Constant decline in conc. (conc vs. time) Rate is independent of [] Rate stays constant in rate vs. conc graph

Obtained by adding all the orders of the reactants

Rate = k [A]^m [B]^n Includes all reactants up to and including the rate determining step May include catalysts

A number that allows the equation to work. It is unchanged by changes to concentration but will increase at higher temperatures

Speed at which a reactant is destroyed Speed at which a product is formed conc/dm^3 s^1

Time it takes for the concentration of a reactant to halve

Reaction that occurs at a much slower rate and requires a much higher activation energy

k = ln (2)/ half life

s^-1 Increases w/ temp

Gradient = m = k

We always take the initial rate as that’s the maximum rate Allows us to make a comparison of the effect of any changes of conditions as the rate changes during the reaction

Measures absorbancy (and loss of colour) and you can see how this changes with conc

mol dm-3 s-1

s-1

mol -1 dm3 s-1

dm6 mol-2 s-1

Chemical requires reaction to stop Physical does not interfere w/ progress

So that the colour change happens as close to the inital rate as possible as the colour change begins when all he S2O8 2- ions have been used up. It is only then the I2 can react w/ the starch

Mechanism adds up to overall If species is both on reactants and products side, cancel out Reactants in rate eqn are reactants of RDS

As T increases as does k and therefore so does the rate If Ea is reduced, k increases For every 10 degree rise in T, k is doubled as is the rate T and k have a +ve exponential relationship