• Autocatalysis the term used to describe a reaction which is speeded up by a product which acts as a catalyst for the reaction
• If you plot a rate graph of concentration versus time it has an usual shape

Concentration versus time for an autocatalytic reaction

• The gradient becomes steeper during the course of the reaction which tells you the rate is speeding up, not slowing down over time as the reactants become used up
• An example of an autocatalysed reaction takes place between?manganate(VII)?ions and?oxalate?(ethandioate) ions
• The overall equation can be deduced from the half equations

• You can see that one of the products is manganese(II) ions - this is the catalyst
• As more manganese(II) is formed the reaction speeds up
• Like to the role of iron(II) in the previous section, manganese(II) ions take part in a redox cycle between two different oxidation states (+2?→??+3?→?+2)

4Mn2+?(aq)??+??MnO4–?(aq) + 8H+?(aq)? ?→? ?5Mn3+?(aq) ?+ 4H2O (aq)

2Mn3+?(aq)??+??C2O42-?(aq)? →? 2CO2?(g) +? 2Mn2+?(aq)

• The manganese(II) is not present in the beginning of the reaction, but as it is formed is speeds up the reaction and is re-generated during the redox cycle
• This reaction is easily followed on a colorimeter as the rate at which the purple manganate(VII) ion is consumed accelerates with time