[EndlessDelusion]

The minimum activation energy for temperature to double a reaction using the 10 degree rule.

Sorry for the long title.. but It's a hard one to cram into the subject bar.
I'm writing some chemistry A2 coursework and finishing the fine details: I'm finding it hard to find information for the 10 degree rule on doubling the rate of an equation. This only works with some reactions and not others. With the reactions that DO change reaction speed every 10 degrees, what is the minimum activation energy required for these reactions to be true?

Thanks for any *delete me*

[JimClark]

This doubling of reaction rate for a 10 degree rise "rule of thumb" works for reactions with activation energies of about 50 kJ/mol within a few tens of degrees of room temperature.  If you know the activation energy for the reaction, you can calculate the effect of increasing the temperature for any particular reaction from the Arrhenius Equation (at least to a reasonable approximation).

You will find this discussed on the Chemguide page http://www.chemguide.co.uk/physical/basicrates/arrhenius.html