The catalytic decomposition of N2O(g) by gold at 900oC and at an initial pressure of 200mm is 50% completed in 53 minutes and 73% completed in 100 minutes. (i) What is the order of the reaction? (ii) Calculate the velocity constant. (iii) How much of N2O(g) will decompose in 100min, at the same temperature but at initial pressure of 600 mm

The catalytic decomposition of N2O(g) by gold at 900oC and at an initial pressure of 200mm is 50% completed in 53 minutes and 73% completed in 100 minutes.
(i) What is the order of the reaction?
(ii) Calculate the velocity constant.
(iii) How much of N2O(g) will decompose in 100min, at the same temperature but at initial pressure of 600 mm

Solution=
50% completed in approx 50 min,

to get the order-

Kt=2.303logAo/Ao−x

K=2.30350log100/50

k=.013min−1
(i)hence the value of k is constant so the order of reaction is 1.

(ii)Velocity constant = .013min−1

(iii)As the first order reaction does not depend upon the initial conc. so it will decompose the same.