Rates of reaction - kinetics (A2)
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I am looking for research sites (background information) on the reaction between hydrogen peroxide and iodide ions but can't seem to find any could you suggest any please?
Also how do I calculate the amount of hydrogen peroxide (20 Vol = 1.8 mol dm-3)
to dilute down to a concentration of 0.25 mol dm-3?
What formula would I need to use to calculate the amount of hydrogen peroxide measured out to be diluted.
010208
Corrie writes......
Let's say you want to make 1 dm3 of 0.25 mol dm-3 peroxide solution. This will contain 0.25 mol of H2O2.
The volume of 1.8 mol dm-3 ('20 volume') peroxide containing 0.25 mol of H2O2 is:
Volume = (0.25 x 1000)/1.8 = 139 cm3 - - -[from: moles = (vol/1000) x conc]
If you measure out this volume of 20 volume peroxide solution and make it up to 1 dm3, then the result should be a 0.25 mol dm-3 solution. Check if I am correct by calculating the new concentration.
You can find some information about the peroxide/iodide reaction (a type of 'clock' reaction, also called the Harcourt-Esson reaction) by typing some of these terms into Google. You could also type 'hydrogen peroxide' into Re:act's Search - quite a few past FAQs will turn up, some involving this reaction with iodide.
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updated: 01 February 2008
