Answer:
First order
Explanation:
Hello,
For this question, the general rate law must be considered:
[tex]\frac{d[N_2O_5]}{dt} =-k[N_2O_5]^n[/tex]
By linearizing it, one could get:
[tex]ln(\frac{d[N_2O_5]}{dt})=ln(k)+nln([N_2O_5])[/tex]
Whereas n stands for the order of the reaction and k the rate constant. For it, I attached an Excel doc for you to see the linearization, in which the slope matches with n, which has a value of 0.999 (neglecting the both the inital and final data otherwise the result is nearly 0.93), thus one could state that the order of the reaction is: first order.
Note: the differential is found by using the centered differentiation formula (Chapra, numerical analysis).
Best regards.
