Raising the temperature 10°C for many reactions would double the reaction rate under what conditions?

So, I am having trouble with my Chemistry lab. Can someone help me out? It also says to use the Arrhenius equation [k = Ae^(–Ea/RT)], which allows us to compute the reaction rate constant as a function of absolute temperature.

Raising the temperature 10°C for many reactions would double the reaction rate under what conditions?
I believe you need to assume an average activation energy (Ea) for a typical organic reaction (the value of 20kcal/mole seems to stick in my mind, but don't take it as "gospel"). You can then plug in values of T that are different by 10 C and see if the resulting rate approxamately doubles. Note: you need to use temps in K for this to work. I would suggest trying "reasonable" values of T near room temperature as this "rule of thumb" might not hold at extreme temperatures.





I hope this helps!