± The Arrhenius Equation
The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as
k=Ae−Ea/RT
where R is the gas constant (8.314 J/mol⋅K), A is a constant called the frequency factor, and Ea is the activation energy for the reaction.
However, a more practical form of this equation is
lnk2k1=EaR(1T1−1T2)
which is mathmatically equivalent to
lnk1k2=EaR(1T2−1T1)
where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (T1 and T2).
Part A
The activation energy of a certain reaction is 32.9 kJ/mol . At 25 ∘C , the rate constant is 0.0140s−1. At what temperature in degrees Celsius would this reaction go twice as fast?
Part B
Given that the initial rate constant is 0.0140s−1 at an initial temperature of 25 ∘C , what would the rate constant be at a temperature of 130. ∘C for the same reaction described in Part A?
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