The activation energy of a certain reaction is 38.1 kJ/mol . At 26 ∘C , the rate constant is 0.0190s−1. At what temperature in degrees Celsius would this reaction go twice as fast? I got that 40.5 degrees celsius
Given that the initial rate constant is 0.0190s−1 at an initial temperature of 26 ∘C , what would the rate constant be at a temperature of 150. ∘C for the same reaction described in Part A? I got 1.34 s^-1 and 1.43 s^-1 both wrong....not sure where I'm messing up the Arrhenius Equation.
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