Arrhenius Reaction
posted by Amy .
The activation energy of a certain reaction is 32.9 kJ/mol At 25 degrees C the rate constant is 0.0160 units s1 units. At what temperature in degrees Celsius would this reaction go twice as fast?
Given that the initial rate constant is 0.0160 s1 at an initial temperature of 25 degrees C , what would the rate constant be at a temperature of 130 degrees C for the same reaction described in Part A?

What's your trouble with this?
b.
ln(k2/k1) = (Ea/R)(1/T1  1/T2)
ln(k2/0.0160) = (32900/0.08206)(1/298/15  1/403.15)
Solve for k2. 
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