A first order reaction is found to have a pre-exponential or 'frequency factor' A of 6 x 1012 s-1. The activation energy for the reaction is 93 kJ mol-1. Calculate the magnitude of the rate constant for the reaction at 298K?

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Answer 1 · 2018-01-19T23:43:33

The rate constant would be #2.98xx10^(-4)# /s

You need the Arrhenius equation for this problem:

k = #Ae^(-E_a/(RT))#

where R is the gas constant, #8.314xx10^(-3)# (to match the other units in the given values).

Using T=298 and the given value of #E_a#, the exponent is

#-E_a/(RT) = -93/((8.314xx10^(-3))(298)) = -37.54#

The rate constant #k# is

#k = (6xx10^(12))(e^(-37.54)) = 2.98xx10^(-4)# /s