Answer:
k = 0,0025 s⁻¹
Explanation:
To calculate the rate constant it is necessary to find out the order of reaction.
For zeroth order the integrated rate law is:
[A] = [A]₀ -kt
The graph of [A] vs t gives a correlation coefficient R² of 0,9948.
The first order is:
ln [A] = ln [A]₀ -kt
The graph of ln [A] vs t gives a R² of 1
The second order is:
1/[A] = 1/[A]₀ -kt
The graph of 1/[A] vs t gives a R² of 0,9939
As R² = 1 for first order, the descomposition of azomethane follows this kinetics order. The lineal correlation is:
y = b - mx
y = 1,412 - 0,0025x
ln [A] = ln [A]₀ -kt
That means:
-k = - 0,0025 s⁻¹
k = 0,0025 s⁻¹
I hope it helps!
