Question

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).

1. The activation energy of a certain reaction is 30.6 kJ/mol . At 28 ∘C , the rate constant is 0.0170s−1 . At what temperature in degrees Celsius would this reaction go twice as fast?

2. Given that the initial rate constant is 0.0170s−1 at an initial temperature of 28 ∘C , what would the rate constant be at a temperature of 170. ∘C?

Answer 1