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Explanation of Arrhenius Law and Kinetics

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I need help understanding the meaning and units involved in the Arrhenius Law equation.

Assuming a first order reaction:

k = Ae^-Ea/RT

1) Can this be re-written as: logk = -Ea/RT + constant ? What is the constant?

2) In either case:

a) How do I determine or choose the activation energy Ea? Where would I find this value?
b) Similarly, how would I determine the frequency factor A???
c) Is it assumed that the exponent e value is really power 10^-Ea/RT?

I just want to know how I actually plug in values in this equation if I am trying to determine the difference in the rate reaction at temp 1060 degrees K and 673 degrees K

Is k ultimately in units of 1/sec??

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https://brainmass.com/chemistry/chemical-kinetics/explanation-arrhenius-law-kinetics-135618

Solution Summary

Arrhenius Law and its equation are explained. The expert examines first order reaction kinetics.

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