# Question 8c999

Jan 4, 2018

Here are the steps.

#### Explanation:

(a) The order of the reaction

For the reaction $\text{A → Products}$, the rate law is

"Rate" = k["A"]^n

Use experiments 1 and 2 and the method of initial rates to determine the value
of $n$.

(b) The rate constant

Insert your value of $n$ and the data from experiment 1 or 2 and calculate the value of $k$ at 25 °C.

Repeat for experiment 3 and calculate the value of $k$ at 35 °C.

(c) The activation energy

Use the rate constants at 25 °C and 35 °C to calculate (Δlnk)/(Δ(1/T)).

(Δlnk)/(Δ(1/T)) = "-"E_text(a)/R#

Then calculate ${E}_{\textrm{a}}$.