Final answer:
The statement about the best fit line on an Arrhenius plot being directly related to the rate constant having units of L/(mol s) and temperature in K is typically false. The Arrhenius equation relates the rate constant to temperature, activation energy, and frequency factor and involves plotting the natural logarithm of the rate constant against the inverse of temperature.
Step-by-step explanation:
The student's question pertains to the Arrhenius equation, which is used to determine the relationship between the rate constant of a reaction, the activation energy, the frequency factor, and temperature. The claim that the equation of the best fit line on an Arrhenius plot is related to the rate constant (k) having units of L/(mol s) and temperature (T) in K can be true or false depending on the context of the question. However, from the options provided, it is typically false because the Arrhenius plot usually shows the natural logarithm of the rate constant ln(k) versus the inverse of temperature 1/T.
Additionally, the rate law constant k has units that ensure, when multiplied by the concentrations involved in the rate expression, the resultant rate of reaction units are mol/L/s. For a reaction of order n (where n is the sum of the exponents in the rate expression), k will have units of (mol1-n)/(L1-ns).
To determine the activation energy, one would use the slope of the line on an Arrhenius plot, which is represented by -Ea/R. This calculation is essential in understanding how sensitive a reaction rate is to changes in temperature.