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a chemistry question straight from my textbook.. though not really chemistry..?

k here's one of the questions:

in general, it is observed that the rate of a chemical reaction doubles with every 10 degree rise in temperature. if this generalization holds for a reaction in the temperature range 298K - 308K what would be the value of activation energy for this reaction (given that R= 8.314 j/K/mol)

i have to use the arrhenious equation to solve it...and it goes..

log (k2/k1) = Eact/[2.303R] x [1/T1 - 1/T2]

where k1 and k2 are initial and final rate constants resp. ; Eact is the activation energy; R is rydberg's constant ; T1 is initial temperature(298) and T2 is final temperature(308) ...

im not bothered with the sum.. but can anyone guess what my age is. and which year of education i'm doing? (grade 1-12 or 1'st -4th year of uni or masters or whatever) .. best guess gets best answer obviously